A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Ag+ Hg²+ Lit Ba2+ Pb2+ Mg2+ Hgž*

A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Ag+ Hg²+ Lit Ba2+ Pb2+ Mg2+ Hgž*

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

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH. Assume no volume change upon the addition of base. The K, for HF is 3.5 × 104. 3.82 3.22 3.69 4.46 3.09
A buffer is made with 1.0 mol of sodium acetate and 1.0 mol acetic acid in 1 liter of solution. Determine the pH of the solution, and determine the pH of the solution after the addition of 15 mL of 3.0 M sodium hydroxide.
A buffer solution contains 0.368 M NaH₂PO4 and 0.232 M K₂HPO4. Determine the pH change when 0.055 mol HCIO4 is added to 1.00 L of the buffer. pH change = 0.05
An analytical chemist is titrating 103.2 mL of a 0.8800 M solution of propionic acid (HC,H,CO,) with a 0.2500M solution of KOH. The p K, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 421.7 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH =
A buffer is prepared by adding 35 mL of 0.100 M hypochlorous acid, HOCl, to 65 mL of 0.300 M hypochlorite, OCl ̄. What is the pH of the final solution? (the Ka hypochlorous acid of is 3.5 x 10-8)?
A buffer solution contains 0.285 M ammonium chloride and 0.354 M ammonia.If 0.0259 moles of hydroiodic acid are added to 225 mL of this buffer, what is the pH of the resulting solution?(Assume that the volume does not change upon adding hydroiodic acid.)
What you expect to observe on mixing 6M NH3 with HCl. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?
A 23.1 mL sample of 0.382 M ethylamine, C,H;NH,, is titrated with 0.297 M hydrobromic acid. The pH before the addition of any hydrobromic acid is
A student receives an unknown mixture that is thought to contain the Group I cations. The student performs qualitative analysis on the sample and makes the folowing observa -After adding excess Nact a precipitate was formed. - After the mixture was heated and decanted, a precipitate was seen when the heat was removed. With the addition of ammonia to the tube containing the precipitate, no color change was observed. -No white precipitate was formed after the addition of the pH 4 solution to the test tube Which of the Group I cations are likely to be present? Choose all that apply. DANa B. Ag OC. No Group I cations are present in this mixture □D-Hg₂+ E.Pb2+ OF. Hg2+
Consider the titration of 50.0 mL of 0.134 M HNO3 with 0.0500 M KOH. What is the initial pH of HNO3 before any KOH has been added?
A buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of 0.500 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid. pKa of HNO2 is 3.40 Ka of HNO2 is 4.0E-4 m.w. of HNO2 is 47.01 g/mol pH of the buffer solution is 3.30, so now Calculate the pH of the buffer solution after the addition of 5.00 ml of 2.50 M Ba(OH)₂.
2. Identify those salts that are more soluble in acid than in neutral solution. Explain why. ZNCO3 Ni(OH)2 Agl AIPO4 PbCl2 Hg2Br2 CuS