A student attempts to identify six solutions that contained either hydrogen peroxide (H202), calcium chloride, calcium acetate, lithium acetate, lithium hydroxide, or lithium permanganate. The tests performed were conductivity, solution colour, flame colour, and the addition of lead(II) nitrate solution. The following evidence was collected: Flame Solution Addition of Conductivity Solution Colour Colour РЬ(NO3)2(ag) yellow- White precipitate yes colourless red forms hydrogen peroxide calcium chloride No precipitate forms yes red purple calcium acetate lithium acetate No precipitate forms lithium hydroxide lithium permanganate none none colourless White precipitate yes red colourless forms No precipitate yes red colourless forms yellow- No precipitate yes colourless red forms

A student attempts to identify six solutions that contained either hydrogen peroxide (H202), calcium chloride, calcium acetate, lithium acetate, lithium hydroxide, or lithium permanganate. The tests performed were conductivity, solution colour, flame colour, and the addition of lead(II) nitrate solution. The following evidence was collected: Flame Solution Addition of Conductivity Solution Colour Colour РЬ(NO3)2(ag) yellow- White precipitate yes colourless red forms hydrogen peroxide calcium chloride No precipitate forms yes red purple calcium acetate lithium acetate No precipitate forms lithium hydroxide lithium permanganate none none colourless White precipitate yes red colourless forms No precipitate yes red colourless forms yellow- No precipitate yes colourless red forms

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the molar solubility of Ga(OH)3 (Kp 7.28 x 10 36) in a solution that is buffered at pH = 3.22.
The student added universal indicator to the alkali solution at the start of the experiment. The indicator changed colour when the acid was added to the alkali. Explain how the student used this information and the pH scale to explain that this is a neutralisation reaction.
The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O O
You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.
Calculate the initial concentration of Fe3+, based on the dilution that results from adding KSCN solution and water to the original 0.0020 M Fe(NO3)3solution. See Step 2 of the procedure for the volume of each substance used in Test Tubes 1-4. This value will be the same value for all four test tubes. This is essentially the same as filling out part of the “I” row in an ICE table. Test tube number 0.0020 M Fe(NO3)3(mL) 0.0020M KSCN(mL) H2O(mL) 1 5 2 3 2 5 3 2 3 5 4 1 4 5 5 0
Upon analyzing a seawater sample, it was found that the concentration of bicarbonate ions (HCO3-) is 0.09 m, the activity of calcium ions (Ca2+) is 10^-6, and the pH of the seawater sample is 8.0. (a) Will calcite precipitate in this seawater sample? (b) Calculate the required activity of Mg2+ ions for dolomite to precipitate.
What will be the solubility product constant, Qsp, for the reaction of 64.5 mL of 0.045 M Ni(NO3)2 and 85.5 mL of 0.025 M Li2CO3? Ni(NO3)2 (aq) + Li2CO3 (aq) →
For a 50ml beaker, 0.4532g of pure iron III oxide was weighed, to which 1 ml of a concentrated hydrochloric acid solution was added and then 20 ml of deionized water was added to the beaker. After mixing, the resulting solution was transferred to a 50.00 ml flask and the volume was made up with deionized water. Then 15ml of this solution into a second beaker to which 10ml of an iron iii chloride solution of 0.200 M concentration was added. Calculate the final concentration of the iron iii cation solution expressed in mol/L and in g/L, considering that the volumes are additive.
Write a balanced net ionic equation to show why the solubility of Mg(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). Mg(OH)2(s) + 2HCl(aq) MgCl2(aq) + 2H2O(l) K =