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Question 1 Report
Which of the following species correctly represented an ion of M with 13 protons and 10 electrons?
Answer Details
An ion is an atom or molecule that has lost or gained one or more electrons and has a net electric charge. In this question, the element M has 13 protons and 10 electrons, which means it has a net charge of +3 to balance out the charges of the protons and electrons. Therefore, the correct answer is 13M 3+. The other options are incorrect because they either have the wrong number of protons or the wrong number of electrons to match the given element.
Question 2 Report
Which of the following metals exists as liquid at ordinary temperature?
Answer Details
Mercury is the only metal among the given options that exists as a liquid at ordinary temperature. Copper, gold, and silver are all solid at room temperature and require high temperatures to melt and become liquid. Mercury, on the other hand, has a melting point of -38.83°C and a boiling point of 356.73°C, making it liquid at room temperature. Therefore, the correct answer is "Mercury".
Question 3 Report
Which of the following statements about chlorine and iodine at room temperature is correct?
Answer Details
Chlorine and iodine are both nonmetals that exist as diatomic molecules, which means they are made up of two atoms of the same element. At room temperature (around 25°C or 77°F), chlorine is a yellow-green gas, while iodine is a shiny black or purple solid. Therefore, the correct statement is: "Chlorine is a gas and iodine is a solid."
Question 4 Report
A solution of sodium trioxocarbonate (IV) contains 10.6g in 250cm3 of solution. Calculate the concentration of the solution. [Na2CO3 = 106.0]
Answer Details
To calculate the concentration of the sodium trioxocarbonate (IV) solution, we need to use the formula: Concentration (in mol dm-3) = (mass ÷ molar mass) ÷ volume Firstly, we need to calculate the number of moles of Na2CO3 in the solution: mass of Na2CO3 = 10.6 g molar mass of Na2CO3 = 106.0 g mol-1 Number of moles of Na2CO3 = mass/molar mass = 10.6/106.0 = 0.1 mol Next, we can use the formula above to calculate the concentration: Concentration (in mol dm-3) = (mass ÷ molar mass) ÷ volume Volume = 250 cm3 = 0.25 dm3 Concentration (in mol dm-3) = (0.1 mol ÷ 0.25 dm3) = 0.4 mol dm-3 Therefore, the concentration of the sodium trioxocarbonate (IV) solution is 0.4 mol dm-3. The correct option is (A) 0.4 mol dm-3.
Question 5 Report
Consider the neutralization reaction represented by the following equation: Na2CO3 + 2HNO 3 → 2NaNO3 + H2O + CO2 The stoichiometric ratio of acid to base is
Answer Details
The stoichiometric ratio of acid to base refers to the ratio of the coefficients of the acid and base in a balanced chemical equation. In the given equation, the balanced equation is: Na2CO3 + 2HNO3 → 2NaNO3 + H2O + CO2 The coefficients of HNO3 and Na2CO3 are 2 and 1 respectively. Therefore, the stoichiometric ratio of acid to base is 2:1. This means that for every 2 moles of HNO3 used in the reaction, 1 mole of Na2CO3 reacts.
Question 6 Report
The minimum amount of energy required for effective collisions between reacting particles is known as
Answer Details
The minimum amount of energy required for effective collisions between reacting particles is known as "activation energy." In simple terms, it is the energy required to start a chemical reaction by breaking the bonds of the reactants. It is the energy barrier that needs to be overcome before a chemical reaction can occur. Once this energy barrier is overcome, the reaction proceeds on its own, releasing energy in the form of heat or light. The activation energy is dependent on the nature of the reactants and the reaction conditions such as temperature and pressure.
Question 7 Report
Compound N reacts with sodium metal to produce a gas that gives a 'pop' sound with a burning splint N also react with ethanoic acid to give a sweet smelling liquid. Compound N is an
Question 10 Report
The products of fermentation of sugar are
Answer Details
The correct answer is "ethanol and carbon (IV) oxide". Fermentation is a metabolic process that converts sugar (glucose) into alcohol (ethanol) and carbon dioxide through the action of enzymes in the absence of oxygen. The reaction is catalyzed by yeast or bacteria, which break down the glucose molecule into two molecules of pyruvate in a process called glycolysis. Pyruvate then undergoes further chemical reactions that produce ethanol and carbon dioxide as waste products. The balanced chemical equation for the fermentation of glucose is: C6H12O6 → 2 C2H5OH + 2 CO2 So, the products of fermentation of sugar are ethanol and carbon dioxide.
Question 11 Report
A solid substance with high melting and boiling points is likely to be a/an
Answer Details
A solid substance with high melting and boiling points is likely to be an electrovalent compound. Electrovalent compounds (also known as ionic compounds) are formed by the transfer of electrons between a metal and a non-metal, resulting in the formation of a lattice structure held together by strong electrostatic forces between positively and negatively charged ions. These strong intermolecular forces make it difficult to break the lattice structure, leading to high melting and boiling points. Covalent compounds, on the other hand, typically have weaker intermolecular forces, resulting in lower melting and boiling points. Dative covalent compounds are a type of covalent compound where both electrons in a shared pair are donated by one atom, and non-metals are a broad category of elements that can form both covalent and electrovalent compounds.
Question 12 Report
An organic compound contains 40.0% carbon, 6.7% hydrogen and 53.3% oxygen. What is the empirical formula of the compound? [O = 16.0, C = 12.0, H = 1.0]
Answer Details
To determine the empirical formula of the compound, we need to find the simplest whole number ratio of the atoms present in the compound. Assume we have 100g of the compound. This means that we have: - 40.0g of Carbon - 6.7g of Hydrogen - 53.3g of Oxygen Next, we need to convert the mass of each element to moles. We can do this by dividing the mass of each element by its atomic weight: - Moles of Carbon = 40.0g ÷ 12.0g/mol = 3.33 moles - Moles of Hydrogen = 6.7g ÷ 1.0g/mol = 6.7 moles - Moles of Oxygen = 53.3g ÷ 16.0g/mol = 3.33 moles We can then divide each of the mole values by the smallest mole value to get the simplest whole number ratio: - Carbon: 3.33 ÷ 3.33 = 1 - Hydrogen: 6.7 ÷ 3.33 = 2.01 (approx. 2) - Oxygen: 3.33 ÷ 3.33 = 1 Therefore, the empirical formula of the compound is CH2O. The correct answer is (c) CH2O.
Question 13 Report
The following substances are normal salts except
Answer Details
A normal salt is formed by the complete replacement of the hydrogen ions of an acid by a metal ion or ammonium ion. Ammonium salts are also normal salts. Out of the given options, all are salts except for Mg(OH)NO3, which is a complex salt. This is because Mg(OH)2 is a weak base and reacts partially with nitric acid to form a complex salt, which contains the anions of both Mg(OH)2 and HNO3. Thus, the correct answer is Mg(OH)NO3.
Question 14 Report
Which of the following molecules has a linear shape?
Answer Details
A molecule is linear if all of its atoms lie in a straight line. Of the given molecules, only CO2 has a linear shape because it has a central carbon atom double-bonded to two oxygen atoms, which are both linearly arranged on opposite sides of the carbon atom, forming a straight line. CH4, H2S, and NH3 have a tetrahedral, bent, and pyramidal shape respectively, meaning they are not linear.
Question 15 Report
Which of the following apparatuses can be used to measure accurately a specific volume of a liquid?
Answer Details
A measuring cylinder can be used to measure accurately a specific volume of a liquid. Measuring cylinders have graduated scales on the side, which allow for precise measurement of the volume of a liquid. They come in different sizes and are often used in experiments where the volume of a liquid needs to be measured with a high degree of accuracy. Beakers and conical flasks, on the other hand, do not have precise measurement markings and are therefore not ideal for accurately measuring specific volumes of liquids. Pipettes, however, can also be used to accurately measure a specific volume of a liquid, and are often used when very precise measurements are required.
Question 16 Report
Which of the following statements about the electrolysis of CuSO4(aq) using copper cathode and platinum anode is not correct?
Question 17 Report
The quantity of electricity required to discharge 1 mole of univalent ion is
Answer Details
The quantity of electricity required to discharge 1 mole of univalent ion is known as the Faraday constant, which is equal to the charge of 1 mole of electrons and has a value of approximately 96,500 coulombs (C). This means that the correct answer is, 96,500 C. Therefore, to discharge 1 mole of univalent ions, a charge of 96,500 C is required.
Question 18 Report
Which of the following factors would not affect the solubility of a gas?
Question 20 Report
Which of the following elements is a d-block element?
Answer Details
Iron is a d-block element. The d-block elements are also known as the transition metals, which are located in the middle of the periodic table between the s-block elements and the p-block elements. Iron (Fe) is a transition metal with an atomic number of 26, and it is located in the d-block. The d-block elements have partially filled d-orbitals, which give them unique properties such as variable oxidation states, colorful complexes, and catalytic activity.
Question 21 Report
Which of the following equations represents beta decay?
Answer Details
The correct equation that represents beta decay is: \(\frac{8238}{92}\)U → \(\frac{239}{93}\)Np + \(\frac{0}{-1}\)e In beta decay, a neutron in the nucleus of an atom breaks down into a proton and an electron. The electron is then emitted from the nucleus, and the proton remains in the nucleus. This results in the atomic number of the nucleus increasing by one, but the mass number remaining the same. The equation above represents the beta decay of Uranium-238 into Neptunium-239 by the emission of an electron (0/-1 e).
Question 22 Report
Consider the equilibrium reaction represented by the following equation: 2SO2(g) + O2(g) ⇌ 2SO3(g); ∆H = 395.7 kJmol-1 Which of the following statements about the equilibrium system is correct?
Question 23 Report
Which of the following oxides is basic?
Answer Details
Out of the given options, CaO is a basic oxide. Basic oxides are also called alkaline oxides or simply bases, which have a pH value greater than 7. When they react with water, they produce metal hydroxides, which are also bases. CaO, or calcium oxide, is a metal oxide that reacts with water to produce Ca(OH)2, which is a strong base. In contrast, NO2 and SO2 are acidic oxides, and Al2O3 is an amphoteric oxide, which means it can behave as either an acid or a base depending on the conditions.
Question 24 Report
Which of the following substances cannot be classified as a heavy chemical?
Question 25 Report
Which of the following chlorides is insoluble in water?
Answer Details
Among the given options, AgCl is the only chloride that is insoluble in water. This is because AgCl has a very low solubility in water, which means that only a small amount of it can dissolve in water. In contrast, KCl, NH4Cl, and ZnCl2 are all soluble in water, meaning they can easily dissolve in water to form a homogeneous solution. The solubility of a salt in water depends on various factors such as the nature of the ions, temperature, and pressure.
Question 26 Report
The energy change which accompanies the addition of an electron to a gaseous atom is
Answer Details
The energy change which accompanies the addition of an electron to a gaseous atom is called "electron affinity". In simple terms, it is the energy released or absorbed when a neutral gaseous atom gains an electron to form a negatively charged ion. This energy change is often expressed in units of kilojoules per mole (kJ/mol). A positive electron affinity value indicates that energy is absorbed when an electron is added, whereas a negative value indicates that energy is released.
Question 27 Report
What is the change in oxidation number of manganes in the reaction represented by the following equation? MnO-4(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l)
Answer Details
In the given redox reaction, the oxidation state of manganese (Mn) changes from +7 in MnO4- to +2 in Mn2+. Therefore, the change in oxidation state of manganese is from +7 to +2. The oxidation state is the hypothetical charge that an atom would have if all bonds to atoms of different elements were completely ionic. When an element undergoes oxidation, its oxidation state increases, and when it undergoes reduction, its oxidation state decreases. In this reaction, manganese is undergoing reduction since its oxidation state is decreasing from +7 to +2, which means it is gaining electrons.
Question 29 Report
The determination of heat of combustion is carried out with
Answer Details
The determination of heat of combustion involves measuring the amount of heat energy released when a substance is burned completely in oxygen. To measure this energy, a device called a bomb calorimeter is used. The substance is placed in a sealed container (the "bomb"), and then ignited by an electric spark. As the substance burns, the heat produced raises the temperature of the surrounding water, which is used to calculate the heat of combustion. Therefore, the correct answer is "a bomb calorimeter."
Question 30 Report
Which of the following substances is that detergents
Answer Details
The substance that is a detergent and meets the criteria given is "lather readily with water." This is because detergents are a type of surfactant that lowers the surface tension of water, allowing it to penetrate and lift away dirt and oil from surfaces. One of the characteristics of detergents is that they produce foam or lather when mixed with water, which helps to distribute the detergent evenly and aid in cleaning. Therefore, the correct option is "lather readily with water."
Question 31 Report
The main function of limestone in the blast furnance is to
Answer Details
The main function of limestone in the blast furnace is to remove impurities from the iron ore being smelted. Limestone, which is mostly calcium carbonate, reacts with the impurities in the iron ore to form slag, which is then easily separated from the molten iron. The chemical reaction is as follows: CaCO3(s) + SiO2(l) → CaSiO3(l) + CO2(g) Thus, limestone acts as a flux, a substance that can lower the melting point of the iron ore and helps to remove impurities from the ore. It does not act as a reducing agent, catalyst, or supply carbon (IV) oxide.
Question 32 Report
Which of the following molecules has a triple bond in its structure?
Answer Details
Out of the given options, only N2 has a triple bond in its structure. A triple bond is a type of covalent bond in which three pairs of electrons are shared between two atoms. In the case of N2, the two nitrogen atoms share three pairs of electrons, resulting in a triple bond between them. The other options do not have a triple bond in their structure. CH4 has four single covalent bonds, NH3 has three single covalent bonds, and O2 has a double bond between the two oxygen atoms.
Question 33 Report
Which of the following gases contains the highest number of atoms at s.t.p?
Answer Details
At standard temperature and pressure (STP), which is defined as a temperature of 273 K (0°C) and a pressure of 1 atm (101.3 kPa), all gases occupy the same volume of 22.4 L per mole. Therefore, the number of atoms present in a gas is directly proportional to the number of moles of that gas. Thus, the gas with the highest number of atoms at STP would be the one with the highest number of moles. Using Avogadro's law, 1 mole of any gas at STP contains approximately 6.02 x 10^23 atoms or molecules. - 6 moles of neon would contain 6 x (6.02 x 10^23) atoms = 3.61 x 10^24 atoms - 3 moles of oxygen would contain 3 x (6.02 x 10^23) atoms = 1.81 x 10^24 atoms - 2 moles of chlorine would contain 2 x (6.02 x 10^23) atoms = 1.20 x 10^24 atoms - 1 mole of ethane (C2H6) would contain 1 x (2 x 6.02 x 10^23) atoms = 1.20 x 10^24 atoms Therefore, the gas with the highest number of atoms at STP is neon with 6 moles, which contains 3.61 x 10^24 atoms.
Question 34 Report
Which of the following statements about the cell notation Mg/Mg2+//Cu2+/Cu is correct?
Question 35 Report
If X is a group lll element, its oxide would be represented as
Answer Details
Group III elements form oxides in which the oxidation state of the metal ion is +3. The chemical formula for these oxides is M2O3, where M represents the Group III element. Therefore, the oxide of a Group III element X would be represented as X2O3. Option (c) is the correct answer.
Question 36 Report
The rate of chemical reaction of solids are not affected by
Question 37 Report
A given volume of oxygen diffused through a porous partition in 8 seconds. How long would it take the same volume of carbon (IV) oxide to diffuse under the same condition? [C = 12.0, O = 16.0]
Question 38 Report
What is the volume occupied by 2 moles of ammonia at s.t.p?
Answer Details
The volume occupied by 1 mole of any ideal gas at standard temperature and pressure (STP) is 22.4 dm3 or 22.4 L. STP is defined as a temperature of 273 K (0 °C) and a pressure of 1 atm (101.325 kPa). Therefore, the volume occupied by 2 moles of ammonia at STP would be: V = 2 × 22.4 dm3 = 44.8 dm3 So the correct option is (a) 44.8 dm-3.
Question 39 Report
(a) i) Give the name and nature of the radiations that are emitted during radioactivity.
ii) State two differences between chemical reaction and nuclear reaction.
iii) Balance the following nuclear reactions and identify X and Y.
I. \(^{212}_{84} PO\) \(\to\) \(^{208}_{82} Pb\) + X
II \(^{137}_{55}Cs\) \(\to\) \(^{137}_{55}Ba\) + Y
(b) The electron configuration of an element X is: 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^5\)
(i) Deduce the atomic number of X.
(ii) To what group does X belong?
(iii) Give two properties of the group to which the element X belong.
(iv) Identify element X by name.
(v) Write a balanced equation to represent the reaction between the element X and hot concentrated NaOH.
(c)(i) Explain why: I. graphite is used as a lubricant; II. diamond is used as an industrial cutting tool.
(ii) Write an equation to represent the reaction between aqueous HCI and NH\(_3\) solution.
(iii) Name the type of reaction represented by the equation.
Answer Details
None
Question 40 Report
(a) (i) Define a base according to Arrhenius concept.
(ii) Give one example of an Arrhenius base.
(iii) Identify each of the following substances in aqueous solutions as strong electrolyte, non-electrolyte or weak electrolyte.
I. C\(_{12}\)H\(_{22}\)O\(_{11}\) II. NH\(_3\) Ill. NaOH
(iv) Write a balanced equation to represent the reaction between CH\(_3\)COOH and KOH.
(b) Calculate the volume of 0.500 mol dm\(^{-3}\) HCI required to neutralize 20.00 cm\(^3\) of 0.300 mol dm\(^{-3}\) NaOH.
(c) Give the IUPAC name of each of the following salts: (ii) NaOCI; (iii) Mg(HCO\(_3\))\(_2\).
(d)(i) Define the term standard solution.
(ii) Consider the following compounds: NaOH and Na\(_2\)CO\(_3\). Which of the compounds is suitable for the preparation of a standard alkaline solution? Give reason for your answer
(iii) Fe completely reacted with dilute HCI.
I. Write an equation for the reaction
II. If 3.08g of Fe completely reacted with 50.0 cm\(^3\) of 2.20 mol dm\(^{-3}\) HCI, calculate the relative atomic mass of the metal.
Answer Details
None
Question 41 Report
(a (i) Explain why water is referred to as a universal solvent.
(ii) Give one chemical test for water. H\(_2\)SO\(_4\)
(b) A current of 1.25A was passed through an electrolytic cell containing dil. for 40 minutes.
(i) Write (ii) Calculate the volume of gas produced at the anode at s.t.p. (1F = 96,500 C, Molar Volume of gas at s.t.p. = 22.4 dm\(^3\) mol\(^{-3}\) ]
(C) Consider the reaction represented by the following equation: Au\(_{(s)}\) + Cl\(_{2(g)}\) \(\to\) AuCl\(_{3(s)}\)
(I) Balance the equation
(ii) If 1.2509 of Au and 1.744g of Cl\(_2\) were mixed
I. determine which of the reactants is in excess II. calculate the excess amount [Au = 197.0, CI = 35.5]
Answer Details
None
Question 42 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
(a) An aqueous solution of salt Q was added to excess Sodium trioxocarbonate (V) solution in a test tube. There was effervescence, the test tube became warm and a white precipitate was observed. State three inferences that could be drawn from these observations.
(b) Consider the following salts: NH\(_4\)CI; PbSO\(_4\); NaHCO\(_3\), Cu(NO\(_3\))\(_2\) and ZnCO\(_3\). Select from the list, the salt(s) which;
(i) do not/does not readily dissolve in water;
(i) produce(s) effervescence with dilute mineral acids;
(ii) decompose(s) on heating
(iv) dissolves(s) in water to form an alkaline solution;
(v) sublime(s) on heating.
Answer Details
None
Question 43 Report
(a)(i) Give the two reasons why soda lime is used instead of caustic soda in the preparation of methane.
(ii) List two physical properties of methane.
(iii) A hydrocarbon with a vapour density of 29 contains 82.76% carbon and 17.24% hydrogen. Determine the: I. empirical formula; II. molecular formula of the hydrocarbon. [ H = 1.00 C = 12.00 ]
(b)(i) What is meant by the term isomerism?
(ii) Draw the structures of the two isomers of the compound with the molecular formula C\(_2\)H\(_6\)O.
(iii) Give the name of each of the isomers in (b)(ii).
(iv) State the major difference between the isomers.
(c) Give three deductions that could be made from the qualitative and quantitative analysis of a given organic compound.
(d) Give one chemical test to distinguish between propene and propane.
Answer Details
None
Question 44 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
Burette readings (initial and final) must be given to two decimal places. Volume or pipete used must also be recorded but no account of experimental procedure is required. All calculations must be done in your answer book.
A is a solution containing 12.0g dm\(^{-3}\) NaHSO\(_4\) NaHSO\(_4\) P is a solution containing NaOH
(a) Put A into the burette and titrate it against 20.0cm\(^3\) or 25.0m\(^3\) portions of B using methyl orange as an indicator. Repeat the titration to obtain consistent titres. Tabulate your readings and calculate the average volume A used. The equation for the reaction involved in the titration is ;
NaHSO\(_{4(aq)}\) + NaOH\(_{(aq)}\) \(\to\) Na\(_2\)SO\(_{4(aq)}\) + H\(_2\)O\(_{(l)}\)
[H 1.00, O = 16.0; Na = 23.0, S = 32.0]
(b) From your results and the information provided above calculate the:
(i) concentration of A in mol dm\(^{-3}\)
(ii) concentration of B in mol dm\(^{-3}\)
(iii) mass of Na\(^+\) formed in solution during the titration.
Answer Details
None
Question 45 Report
(a) (i) Define saturated solution.
(ii) Tha solubility of KNO\(_3\) at 20°C was 3.00 mol dm\(^{-3}\) If 67.0g of KNO\(_3\) was added to 250 cm\(^{-3}\) of water and stirred at 20°C, determine whether the solution formed was saturated or not at that temperature. [ KNO\(_3\) = 101.0 ]
(b) (i) Distinguish between dative bond and covalent bond.
(ii) Explain why sugar and common salt do not conduct electricity in the solid state.
(iii) State the type of intermolecular forces present in: I. hydrogen fluoride; II argon.
(iv) Consider the compounds with the following structures. S - H ---- N and O - H ---- N In which of the compounds is the hydrogen bend stronger? Give reason for your answer.
(c) (i) State Dalton's Law of Partial Pressure.
(ii) If 200cm of carbon (IV) oxide were collected over water at 18°C and 700 mmHg, determine the volume of the dry gas at s.t.p. [ standard vapour pressure of water at 18°C = 15 mmHg]
Answer Details
None
Question 46 Report
(a) Name one product of destructive distillation of coal that is (i) solid (ii) liquid; (iii) gas.
(b) (i) What is the major component of synthetic gas? (ii) Give one reason why synthetic gas is not a major source of air pollution.
(c) (i) Write a balanced chemical equation for the complete combustion of carbon. (ii) State two: I. physical; II. chemical properties of the product in (c)(i).
(d) (i) Name two allotropes of carbon that are I. crystalline, II. amorphous. (ii) State one use of each of the allotropes named in (d)(i).
(e) (i) By means of balanced chemical equations only, outline the process of manufacture of H\(_2\)SO\(_4\), by contact process.
(ii) State the function of H\(_2\)SO\(_4\) in each of the following reaction equations:
I. C\(_2\)H\(_5\)OH\(_{2(l)}\) \(\to\) C\(_2\)H\(_{4(g)}\);
II. Pb(NO\(_{3(g)}\) + H\(_2\)SO\(_{4(g)}\) —> PbSO\(_{4(s)}\) + 2HNO\(_{3(aq)}\)
Answer Details
None
Question 47 Report
TEST OF PRACTICAL KNOWLEDGE QUESTION
Credit will be given for strict adherence to the instructions, for observations precisely recorded, and for accurate inferences. All tests, observations, and inferences must be clearly entered in your answer book, in ink, at the time they are made.
C and D are inorganic salts. X is a solution of an inorganic compound. Carry out the following exercises on C, D and X. Record your observations and identity any gas(es) involved. State the conclusion drawn from the result or each test.
(a)(i) Add about 5 cm\(_3\) of distilled water to C in a test tube and shake thoroughly, Divide the resulting solution into two portions.
(ii) Put about 2cm\(^3\) of X into a separate test tube and add the first portion of solution in (a)(i) To the second portion of the resulting solution in (a)(i), add few drops of BaCl\(_{2(aq)}\) followed by excess dil. HCI.
(b) Add about 10 cm of distilled water to D in a boiling tube and shake thoroughly.
(i) To about 2 cm\(^3\) portion of the resulting solution in a test tube, add NaOH\(_{(aq)}\) in drops and then in excess
(ii) To another 2 cm\(^3\) portion of the resulting solution add few drops of K\(_2\)CrO\(_{4(aq)}\)
Answer Details
None
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