Compare the solubility of lead chloride in each of the following aqueous solutions: Clear All 0.10 M Pb(NO3)2 More soluble than in pure water. 0.10 M KCI Similar solubility as in pure water. 0.10 M NANO3 Less soluble than in pure water. 0.10 M KCH3CO0

Compare the solubility of lead chloride in each of the following aqueous solutions: Clear All 0.10 M Pb(NO3)2 More soluble than in pure water. 0.10 M KCI Similar solubility as in pure water. 0.10 M NANO3 Less soluble than in pure water. 0.10 M KCH3CO0

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.16QAP

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Compare the solubility of lead chloride in each of the following aqueous solutions:
Clear All
0.10 M Pb(NO3)2
More soluble than in pure
water.
0.10 M KCI
Similar solubility as in pure
water.
0.10 M NANO3
Less soluble than in pure
water.
0.10 M KCH3C00

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Figure 16.3 shows the solubility of AgNO3 in water inunits of moles of AgNO3 per kilogram of H2O. If 255 g of AgNO3 is added to 100 g of water at 95°C and cooledslowly, at what temperature will the solution becomesaturated?
12.49 The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mg of solute/L of solution.)
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A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions. (a) Which acid has the larger equilibrium constant for ionization HA[HA(aq)A(aq)+H+(aq)] or HB[HB(aq)H+(aq)+B(aq)]? (b) What are the equilibrium constants for the ionization of these acids? (Hint: Remember that each solution contains three dissolved species: the weak acid (HA or HB). the conjugate base (A- or B- and the hydrogen ion (H+). Remember that osmotic pressure (like all colligative properties) is related to the total number of solute particles. Specifically for osmotic pressure, those concentrations are described by molarities.)
In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)
. Why does the amount of excess solid solute present in a solution not affect the amount of solute that ultimately dissolves in a given amount of solvent?