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Question 2 Report
The oxidation number of X in \(XO_{4}^{3+}\) is
Answer Details
The oxidation number of an element in a chemical compound is a number that represents the charge that an atom of that element would have if the molecule was completely ionic. In a compound, the sum of all the oxidation numbers must equal the net charge on the molecule. In the case of \(XO_{4}^{3+}\), the oxidation number of X can be determined by using this rule. The net charge on the molecule is +3, which means that the sum of all the oxidation numbers of the atoms in the molecule must equal +3. Since the oxidation number of oxygen is always -2, the oxidation number of X can be calculated as follows: \[X + 4(-2) = +3\] Solving for X, we get: \[X = +5\] Therefore, the oxidation number of X in \(XO_{4}^{3+}\) is +5.
Question 3 Report
Chemical reactions occurs when the colliding reactants have energy that is
Answer Details
Chemical reactions occur when the colliding reactants have energy that is greater than the activation energy. Activation energy is the minimum amount of energy required for a chemical reaction to occur. If the colliding reactants do not have enough energy to meet or exceed the activation energy, the reaction will not take place. In other words, the activation energy acts as a barrier that needs to be overcome for the reaction to proceed. Once the reactants have enough energy to surpass this barrier, they can form new products with a lower energy state than the reactants, which releases energy in the form of heat, light, or other forms of energy. Therefore, only when the colliding reactants have energy greater than the activation energy can they overcome this barrier and form new products with a lower energy state, resulting in a chemical reaction.
Question 4 Report
In a saturated solution at a given temperature, the undissolved solutes are in equilibrium with
Answer Details
In a saturated solution, the undissolved solute particles and the dissolved solute particles are in a dynamic equilibrium. This means that at a given temperature, the rate at which solute particles dissolve into the solvent is equal to the rate at which solute particles come out of solution and reform the solid. Therefore, the undissolved solute particles are in equilibrium with the saturated solution, which is the solution that contains the maximum amount of solute that can dissolve at a given temperature. This equilibrium occurs because the solute particles have reached their maximum solubility limit and are unable to dissolve any further. In summary, the undissolved solute particles are in equilibrium with the saturated solution, not with the solvent or the insoluble solute particles.
Question 5 Report
The following glasswares are used to measure the volume of liquids EXCEPT
Answer Details
The glassware that is NOT used to measure the volume of liquids is a test tube. Test tubes are typically used for mixing and holding small amounts of liquids, but they do not have precise measurement markings like the other glasswares listed. Graduated beakers, pipettes, and burettes have measurement markings and are specifically designed for accurately measuring the volume of liquids.
Question 6 Report
A hydrocarbon contained 14.3% hydrogen. The empirical formula for the hydrocarbon is [H= 1.0, C= 12.0]
Answer Details
The empirical formula of a compound gives the simplest whole number ratio of the elements in the compound. To find the empirical formula of a hydrocarbon, we need to know the percentage of hydrogen in it. In this case, the hydrocarbon contains 14.3% hydrogen. To convert this to a whole number ratio, we divide 14.3 by the atomic weight of hydrogen (1.0), which gives us 14.3. This means that for every 12 atoms of carbon, there are 14.3 atoms of hydrogen. To simplify this to a whole number ratio, we divide both 14.3 and 12 by the greatest common divisor, which is 2. This gives us a ratio of 7:6 for hydrogen to carbon atoms. The empirical formula for the hydrocarbon is therefore \(CH_{2}\), which represents the simplest whole number ratio of hydrogen to carbon atoms in the compound.
Question 8 Report
Halogens generally react with metals to form
Answer Details
Halogens are a group of elements that include fluorine, chlorine, bromine, iodine, and astatine. When halogens react with metals, they tend to form salts. Salts are a type of compound that is formed when an acid and a base react with each other. In the case of halogens and metals, the halogen acts like an acid and the metal acts like a base. The halogen donates an electron to the metal, which forms a positively charged ion, and the halogen becomes negatively charged. These two oppositely charged ions then combine to form a salt. For example, when chlorine reacts with sodium metal, they form sodium chloride, which is table salt.
Question 12 Report
The IUPAC name for the compound \(ClCH_{2}CH_{2}OH\) is
Question 13 Report
Calculate the mass of copper deposited if a current of 0.45A flows through \(CuSO_{4}\) solution for 1hour 15mins. [Cu=64.0, S= 32.0, O =16.0, 1F= 96500C]
Answer Details
Question 14 Report
The name of the compound \(C_{4}H_{9}COOC_{3}H_{7}\) is
Answer Details
The name of the compound \(C_{4}H_{9}COOC_{3}H_{7}\) is "pentyl propanoate".
In naming organic compounds, the longest carbon chain is used as the base name, followed by the name of the functional group. In this case, the longest carbon chain has 5 carbons, so the base name is "pentyl". The functional group is a carboxyl group (-COO-), so the ending is "oate". The base name and the ending are combined to get "pentyl propanoate".
Question 15 Report
The mass of one mole of \((NH_{4})_{2}CO_{3}\) is [O=16.0, N=14.0, C=12.0, H=1.0]
Question 16 Report
Which of the following factors characterize members of the same homologous series?
Answer Details
Members of the same homologous series are characterized by having similar physical properties and a gradual change in chemical properties throughout the series. The successive members also undergo changes in their molecular formula by adding a repeating unit of \(CH_{2}\). This means that although the members may have different molecular formulas, they have a similar structural basis and exhibit similar chemical behaviors.
Question 17 Report
Which of the following statements is correct?
Answer Details
The correct statement is "Ionic compounds in solution would conduct electricity." Explanation: 1. Covalent compounds are formed when two or more non-metal atoms share electrons to form a molecule. They do not readily ionize in solution because they do not contain ions. 2. Covalent compounds consist of molecules made up of atoms bonded together by sharing electrons. These molecules do not contain ions. 3. A hydrogen bond is a type of intermolecular force that occurs between a hydrogen atom and an electronegative atom (usually oxygen, nitrogen, or fluorine) in a different molecule. It is not formed between a metal and a non-metal. 4. Ionic compounds are made up of a metal and a non-metal. When an ionic compound dissolves in water, it dissociates into ions, which can carry an electric charge and conduct electricity. Covalent compounds do not dissociate into ions in solution and do not conduct electricity.
Question 18 Report
Atomic orbital is
Answer Details
An atomic orbital is a region around the nucleus of an atom where electrons are most likely to be found. It is not a physical path that electrons travel around the nucleus, but rather a three-dimensional space that describes the probability of finding an electron at a given location within an atom. Atomic orbitals are characterized by their energy level, shape, and orientation in space. The number and arrangement of electrons in atomic orbitals determine the chemical and physical properties of an element.
Question 19 Report
The oxidation number of nitrogen in \(Pb(NO_{3})_{2}\) is
Answer Details
The oxidation number of an element in a compound represents the charge that the element would have if the compound were a completely ionic compound. The oxidation number of nitrogen in Pb(NO3)2 is +5. This can be determined using the concept of oxidation states, which are assigned to elements based on a set of rules. One of the rules is that the sum of the oxidation states of all the elements in a neutral compound must equal zero. In Pb(NO3)2, the oxidation state of lead (Pb) is +2, since it is a metal and typically has a positive charge in ionic compounds. The sum of the oxidation states of nitrogen (N) and oxygen (O) must then equal -2 to balance out the charge of lead. Since there are three oxygen atoms, each with an oxidation state of -2, the sum of the oxidation states of oxygen is -6. The oxidation state of nitrogen must then be +5 to balance the equation. So, the oxidation number of nitrogen in Pb(NO3)2 is +5.
Question 20 Report
The condensation of two units of glucose will produce a dissacharide with the formula \(C_{12}H_{22}O_{11}\) which is
Answer Details
The condensation of two glucose molecules produces a disaccharide known as maltose, with the chemical formula \( \text{C}_{12}\text{H}_{22}\text{O}_{11} \). During this reaction, an -OH group from one glucose combines with an -H from another glucose, releasing a molecule of water (H₂O) and forming a glycosidic bond between the glucose units. This specific reaction distinguishes maltose from other disaccharides like sucrose, which is formed from glucose and fructose. Therefore, the correct answer is maltose.
Question 21 Report
The reason for the decrease in the atomic size of elements across a period is that
Answer Details
Question 22 Report
Fats and oils can be obtained from any of the following sources except
Answer Details
Paraffin oil is not a source of fats and oils. It is a type of hydrocarbon that is used as a fuel or a lubricant and is not a food source. The other options - animals, groundnuts, and palm kernel - are all sources of fats and oils that can be used for cooking or in the production of various food products.
Question 23 Report
Which of the following substances does not have van der Waals' forces?
Answer Details
Question 24 Report
The purity of a solid sample can best be determined by its
Answer Details
The melting point of a solid sample is the most reliable way to determine its purity. The melting point of a pure substance is a fixed temperature, which is well defined and does not change with time. If there are impurities present in the sample, the melting point will be lower and will not be a fixed temperature. By measuring the melting point, we can determine the purity of the sample. If the melting point is lower than expected, it indicates the presence of impurities in the sample. This is because impurities lower the energy needed to break the bonds holding the solid together, allowing it to melt at a lower temperature.
Question 25 Report
A primary alkanol has a molecular mass of 60. What is the structural formula of the compound? [C= 12.0, H= 1.0, O= 16.0)
Answer Details
Question 26 Report
The use of diamond in abrasives is due to its
Answer Details
The use of diamond in abrasives is due to its hardness. Diamond is one of the hardest naturally occurring substances on Earth, and its hardness makes it ideal for use in abrasive applications. When diamond is used as an abrasive, it can cut through and grind down even the toughest materials, including metals and ceramics. Additionally, diamond is incredibly durable, so it can withstand the wear and tear of abrasive applications better than many other materials.
Question 27 Report
Which of the following arrangements indicates the correct decreasing order of ionization energy of period 3 elements?
Answer Details
Question 28 Report
The property of elements which increases down a group of the periodic table is
Answer Details
The property that increases down a group in the periodic table is the ionic radius. The ionic radius is the size of an atom, measured from the center of the nucleus to the outermost shell of electrons. As you move down a group in the periodic table, the number of electron shells increases, making the atom larger and the ionic radius larger. This is due to the fact that the outermost electrons are farther away from the nucleus and are not held as tightly as the inner electrons. This results in a larger overall size of the atom.
Question 29 Report
The property of a chemical reaction that is affected by the presence of a catalyst is
Answer Details
The property of a chemical reaction that is affected by the presence of a catalyst is the activation energy. Activation energy is the energy required for a chemical reaction to occur. Catalysts are substances that can speed up a chemical reaction by lowering the activation energy required for the reaction to happen. This means that the same chemical reaction that would otherwise require a lot of energy to start, can happen more easily and with less energy input in the presence of a catalyst. Imagine trying to push a heavy object up a hill - it takes a lot of effort and energy to get it started. But if there's a ramp, it becomes much easier to push the object up the hill, and less energy is required. In the same way, a catalyst acts like a ramp for a chemical reaction, making it easier for the reaction to occur with less energy input.
Question 32 Report
The number of atoms present in 2.5moles of a triatomic gas is equivalent to [1mole = \(6.02\times 10^{23}\)]
Answer Details
One mole of a substance contains a specific number of particles, which is called Avogadro's number, represented by \(6.02\times 10^{23}\) particles per mole. Therefore, to find the number of particles present in 2.5 moles of a substance, we can simply multiply Avogadro's number by 2.5: Number of particles = 2.5 moles x Avogadro's number Number of particles = 2.5 x \(6.02\times 10^{23}\) Number of particles = \(1.505\times 10^{24}\) So the answer is option (C) \(1.5\times 10^{24}\), which represents the number of atoms present in 2.5 moles of the triatomic gas.
Question 33 Report
Consider the following reaction equation: \(2NO_{(g)} + O_{{2}{(g)}} \to 2NO_{{2}{(g)}}\). What is the change in the oxidation number of nitrogen?
Answer Details
The oxidation number is a number that represents the number of electrons an atom has gained or lost in a molecule. In the given reaction, the oxidation number of nitrogen changes from +2 to +4. At the beginning of the reaction, nitrogen in NO has an oxidation number of +2, while in NO2 it has an oxidation number of +4. This means that nitrogen has gained two electrons and undergone oxidation. To understand why this is happening, we need to look at the reaction. The reactants are NO and O2, and the product is NO2. The oxygen atoms in the reactants have an oxidation number of 0, while in the product they have an oxidation number of -2. This means that each oxygen atom has gained two electrons and undergone reduction. Since nitrogen has not gained or lost any electrons in the reaction, it is not undergoing reduction or oxidation, but it is participating in the reaction by forming bonds with the oxygen atoms. The change in oxidation number of nitrogen from +2 to +4 is a result of sharing two electrons with each oxygen atom in the product. Therefore, the correct answer is "+2 to +4".
Question 34 Report
Classification of alkanols is based on the
Question 35 Report
Which of the following gases is not acidic?
Answer Details
The gas that is not acidic is CO, or carbon monoxide. Acidity is determined by a substance's ability to donate hydrogen ions (protons), and thus, increase the hydrogen ion concentration in a solution. In general, gases that contain oxygen atoms, such as SO3 and NO2, are more likely to be acidic because oxygen has a greater tendency to form bonds with hydrogen atoms. CO, on the other hand, does not contain oxygen and is not acidic.
Question 36 Report
When water was added to a white anhydrous substance X, the colour changed to blue. X is
Answer Details
The white anhydrous substance X changes color to blue when water is added. This is an indication of a chemical reaction taking place, and the resulting blue color is likely due to the formation of a complex compound. Out of the given options, CuSO4 is a blue compound, also known as copper(II) sulfate, and is commonly used as a colorant and in various industrial applications. When it is dissolved in water, it forms a blue solution due to the hydration of copper ions. Therefore, it is most likely that the anhydrous substance X is CuSO4 because the addition of water resulted in a blue color, which is consistent with the characteristic blue color of CuSO4.
Question 37 Report
Which of the following statements about endothermic reaction is correct?
Answer Details
The correct statement about endothermic reactions is that "heat energy is absorbed." Endothermic reactions are those in which energy is absorbed from the surroundings, usually in the form of heat. This causes the temperature of the surroundings to decrease. Activation energy refers to the energy required to start a chemical reaction, and it can be high or low for both endothermic and exothermic reactions. A catalyst is a substance that speeds up a chemical reaction, but it is not always required for an endothermic reaction. Endothermic reactions can occur reversibly or irreversibly, depending on the specific reaction and conditions. The reversibility of a reaction refers to whether it can proceed in both forward and backward directions.
Question 38 Report
When Magnesium reacts with oxygen, heat is
Answer Details
When magnesium reacts with oxygen, it produces magnesium oxide. During this reaction, energy is released in the form of heat. This means that the reaction is exothermic, and the correct answer is "heat is evolved and the reaction is exothermic."
Question 39 Report
The common feature of reactions at the anode is that
Answer Details
The common feature of reactions at the anode is that oxidation is involved. This means that during the reaction, the anode loses electrons and becomes positively charged. As a result, either a neutral atom or a negatively charged ion is produced. In some cases, the electrode may also dissolve due to the reaction. However, the key feature is always oxidation, which is the process of losing electrons.
Question 40 Report
Which of the following statements is NOT a chemical property of an acid?
Question 41 Report
Petroleum is a non-renewable source of energy because it
Answer Details
Petroleum is a non-renewable source of energy because it cannot be regenerated once it is used up. This means that when we use up all the available petroleum, we cannot create more. Petroleum is formed naturally over millions of years from the remains of plants and animals that were buried underground. Although it may be cheap compared to some other sources of energy, it is not a sustainable option for the future. Unlike renewable sources of energy like solar, wind, and hydro power, which can be replenished naturally, petroleum is finite and will eventually run out if we continue to use it at the current rate. While petroleum can be recycled after use, it is still a finite resource and will eventually be depleted. Therefore, it is important to find alternative sources of energy that are renewable and sustainable.
Question 42 Report
The properties of a good primary standard include the following except
Question 43 Report
Which of the following pairs of gases are pollutants from car exhaust?
Answer Details
Question 44 Report
Soluble salts can be prepared by the following methods except
Question 45 Report
The bond angle in tetrahedral molecules such as tetrachloromethane is
Answer Details
The bond angle in tetrahedral molecules like tetrachloromethane is 109.5°. This is because the molecule has a tetrahedral geometry, which means it has four atoms bonded to a central atom, with the angle between any two adjacent bonds being 109.5°. This angle is also known as the tetrahedral angle and is determined by the repulsion between the bonding pairs of electrons around the central atom. The four bonding pairs of electrons in tetrachloromethane repel each other equally, causing them to arrange themselves in a tetrahedral shape with the bond angle of 109.5°.
Question 46 Report
Which of the following species determines the chemical properties of an atom?
Answer Details
The species that determines the chemical properties of an atom is the electron. This is because electrons are responsible for the bonding of atoms with each other, which determines the chemical properties of a substance. Electrons are negatively charged particles that orbit around the nucleus of an atom. The number of electrons in the outermost shell (valence shell) of an atom determines how it will interact with other atoms, forming chemical bonds. The chemical reactivity and behavior of an atom depend on its valence electrons, which determine the atom's ability to form chemical bonds with other atoms. Therefore, electrons play a crucial role in determining the chemical properties of an atom.
Question 47 Report
If 0.2g of a salt is required to saturate 200\(cm^{3}\) of water at room temperature, what is the solubility of the salt?
Answer Details
Question 48 Report
The real harmful effect of the release of chlorofluorocarbons into the atmosphere is that it eventually causes
Answer Details
The release of chlorofluorocarbons (CFCs) into the atmosphere causes a harmful effect by depleting the ozone layer. The ozone layer is a natural layer of gas in the Earth's stratosphere that protects life on Earth by absorbing harmful ultraviolet (UV) radiation from the sun. CFCs break down ozone molecules, causing the ozone layer to become thinner, which allows more UV radiation to reach the Earth's surface. This can lead to an increase in skin cancer, cataracts, and other harmful effects on plants and animals. Therefore, the real harmful effect of the release of CFCs is that it eventually causes excessive ultraviolet light from the sun to reach the Earth's surface.
Question 49 Report
A 0.1\(moldm^{-3}\) solution of sodium hydroxide was diluted with distilled water to 0.001\(moldm^{-3}\). What is the dilution factor?
Answer Details
Dilution factor
= molarconc.ofdilutedmolarconc.ofundiluted
= 0.0010.1=0.01
Question 50 Report
The seperation of Nitrogen from oxygen using fractional distillation of air is possible because
Answer Details
The separation of Nitrogen from Oxygen using fractional distillation of air is possible because of the difference in their boiling points. Nitrogen has a boiling point of -196°C while oxygen has a boiling point of -183°C. This means that at a certain temperature, oxygen will boil and turn into a gas before nitrogen. By carefully controlling the temperature, we can separate the two gases as they boil at different times. This is known as fractional distillation, which is a process that separates a mixture into its different components based on their boiling points. Therefore, the key factor in separating nitrogen from oxygen is their difference in boiling points, not their density, reactivity, or position in the periodic table.
Question 51 Report
(a)(i) Describe briefly the industrial preparation of ammonia.
(ii) Write a balanced equation for the reaction in (a)(i).
(iii) State one way of increasing the yield of ammonia in 4(a)(i).
(iv) State two uses of ammonia.
(b) Describe briefly, one chemical test for each of the following gases in the laboratory: (i) hydrogen; (ii) carbon (IV) oxide; (iii) oxygen.
(c)(i) State the composition of water gas.
(ii) List two uses of water gas.
(d) Describe briefly a simple experiment to determine the type of hardness in a sample of water.
Question 52 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
All your burette readings (initials and final), as well as the size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer booklet.
State what would be observed if the following reactions are carried out in the laboratory:
(i) methyl orange is dropped into a solution of lime juice:
(ii) hydrogen sulphide gas is bubbled through Iron (III) chloride solution:
(iii) sulphur (IV) oxide gas is bubbled into acidified solution of KMnO\(_4\):
(iv) ethanoic acid is added to a solution of Ka\(_2\)CO\(_3\)
Answer Details
None
Question 53 Report
(a)(i) What is an acid-base indicator?
(ii) Give one example of an acid-base indicator.
(b) State the property exhibited by nitrogen(IV) oxide in each of the following equations:,
(i) 4Cu + 2NO\(_2\) -> 4CuO + N\(_2\) (ii) H\(_2\)O + 2NO\(_2\) --> HNO\(_3\) + HNO\(_2\)
(c)(i) Define enthalpy of combustion..
(ii) State why the enthalpy of combustion is always negative.
(d)(i) Distinguish between a primary cell and a secondary cell.
(ii) Give an example of each of the cells stated in I (d)(i).
(e) Define the term mole.
(f) Calculate the amount of hydrochloric acid in 40.0 cm\(^3\) of 0.40 moldm\(^{-3}\) dilute HCl.
(g) Name two substances which can be used as electrodes during the electroylsis of acidified water.
(h) List two forces of attraction that can exist between covalent molecules.
(i) Name the products formed when butane undergoes incomplete combustion.
(j) Write the electron configuration of \(_{26}\)Fe\(^{3+}\)
Answer Details
None
Question 54 Report
(a) Write the molecular formula of X.
(i) What type of reaction is represented by the equation?
(ii) Consider the following reaction equation: C\(_{12}H_2\) \(\to\) X + C\(_8\)H\(_{18}\)
(iii) Draw the structure of two isomers of X.
(iv) Name the isomers drawn in (a)(iii).
(v) Write a balanced equation for the reaction between X and hydrogen.
(b) Describe one test for fats.
(c) Sulphur (IV) oxide is converted to tetraoxosulphate (VI) acid according to the following equation: 2SO\(_{2(g)}\) + O\(_{2(g)}\) + 2H\(_2\)O\(_{(l)}\) \(\to\) 2H\(_2\)OSO\(_{4(aq)}\). If 1.5 moles of oxgen reacts with sulphur (IV) oxide, calculate the mass of tetraoxosulphate (VI) acid produced. [H = 1.0; O = 16.0; S = 32.0].
(d) Consider the following neutralization reaction:
CH\(_3\)COOH + NaOH \(\to\) CH\(_3\)COONa + H\(_2\)O; \(\bigtriangleup\)H\(_1\)
CH\(_3\)COOH + NH\(_4\)OH \(\to\) CH\(_3\)COONH\(_4\) + H\(_2\)O; \(\bigtriangleup\)H\(_2\)
NaOH + HCl \(\to\) NaCl + H\(_2\)O \(\bigtriangleup\)H\(_3\)
(i) Arrange the enthalphy changes for the reactions in order of increasing magnitude.
(ii) Explain briefly your order in (d)(i).
(e) Consider the following substances. Cu\(_{(s)}\), BeCl\(_2\), NaH\(_{(s)}\), HF\(_{(s)}\)and CCl\(_{4(l)}\). State the substance(s) which;
(i) can conduct electricity;
(ii) is/are soluble in water.
Answer Details
None
Question 55 Report
(a)(i) 1. State the periodic law.
2. What is meant by the term periodic property of elements?
(ii) List three properties of an element which show periodicity.
(iii) Explain briefly how each of the properties listed in (a)(i) in varies across the period.
(b) Defulle relative atomic mass.
(c)(i) What phenomenon is exhibited by an element Z which exist as \(^{35}_{17}Z\) and \(^{37}_{17}X\)
(ii) What accounts for the difference in the mass numbers of the element Z?
(iii) Calculate the relative atomic mass of Z if the percentage abundance of \(^{37}_{17}Z\) is 75%
(d)(i) State the method used for collecting each of the following gases: I. CO II. HCI III. H\(_2\)
(ii) Give a reason for your answer stated in (d)(i) I and II
None
Answer Details
None
Question 56 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
All your burette readings (initials and final), as well as the size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer booklet.
F is 2 mixture of two inorganic salts. Carry out the following exercises on F. Record your observations and identify any gas(es) evolved. State the conclusions you draw from the result of each test.
(a) Put all of F in a beaker and add about 10 cm\(^3\) of distilled water. Stir well and filter. Keep the filtrate and the residue.
(b)(i) To about 2cm\(^3\) of the filtrate. add NaOH\(_{(aq)}\) in drops and then in excess.
(ii) To another 2cm\(^3\) portion of the solution, add a few drops of NH3\(_{(aq)}\) in drops and then in excess.
(c) To about 2cm\(^3\) of the solution, add a few drops of HNO\(_{3(aq)}\) followed by few drops of the drops of AgNO\(_{3(aq)}\)
(d)(i) Put all the residue into a clean test-tube and add HNO\(_{3(aq)}\)
(ii) To a portion of the solution from (d)(i)) add NaOH\(_{(aq)}\) in drops and then in excess.
Answer Details
None
Question 57 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
All your burette readings (initials and final), as well as the size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer booklet.
A is 0.200 moldm\(^3\) of HCl. C is a solution containing 14.3g of Na2CO\(_{3}\).xH\(_2\)O in 500 cm\(^3\) of solution.
a) Put A into the burette and titrate it against 20.0 cm\(^3\) or 25.0cm\(^3\) portions of C using methyl orange as indicator. Repeat the titration to obtain Consistent titre values. Tabulate vour results and calculate the average volume of A used. The equation for the reaction is;
Na\(_2\)CO\(_3\) . xH\(_2\)O + 2HCl\(_{(aq)}\) \(\to\) 2NaCl\(_{(aq)}\) + CO\(_{2(g)}\) + (x + 1)\(_3\)H\(_2\)O\(_{(l)}\)
(b) From your results and the information provided. calculate the:
(i) concentration of C in moldm\(^{-3}\)
(ii) concentration of C in gdm\(^{-3}\)
(iii) molar mass of Na\(_2\)CO\(_3\) . xH\(_2\)O
(iv) the value of x in Na\(_2\)CO\(_3\) . xH\(_2\)O. [H =1.0; C = 12.0; O = 16.0; Na = 23.0]
Credit will be given for strict adherence to the instruction, for observations precisely recorded and for accurale references. All tests. obsenations and influences must be cleary entered in the booklet in ink at the same time they are made.
Question 58 Report
(a)(i) Describe briefly how trioxonitrate (V) ions could be tested for in the laboratory.
(ii) State two uses of each of the following compounds: I. sodium chloride; II. sodium trioxocarbonate (IV).
(b) Write balanced equations for the reactions involved in the extraction of iron in the blast furnace.
(ii) State Faraday's first law of electrolysis.
(iii) State two applications of electrolysis.
(c) Concentrated tetraoxosulphate (VI) acid is added to sugar crystals in a beaker. State what would be observed. Explain briefly your answer.
(d) Write an equation for the reaction of zinc powder with:
(i) dilute tetraoxosulphate (VI) acid;
(ii) concentrated tetraoxosulphate (VI) acid.
(e) What property of concentrated tetraoxosulphate (VI) acid is shown in (d)(ii)
Answer Details
None
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