Problem 71
(a) Determine the chloride ion concentration in each of the following solutions: \(0.150 \mathrm{M} \mathrm{BaCl}_{2}, 0.566 \mathrm{M} \mathrm{NaCl}\), \(1.202 \mathrm{M} \mathrm{AlCl}_{3}\) (b) What is the concentration of a \(\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}\) solution that is \(2.55 \mathrm{M}\) in nitrate ion?
Problem 72
(a) What is the \(\mathrm{Na}^{+}\) concentration in each of the following solutions: \(3.25 M\) sodium sulfate, \(1.78 M\) sodium carbonate, \(0.585 \mathrm{M}\) sodium bicarbonate? (b) What is the concentration of a lithium carbonate solution that is \(0.595 M\) in \(\mathrm{Li}^{+} ?\)
Problem 73
Determine the resulting nitrate ion concentration when \(95.0 \mathrm{~mL}\) of \(0.992 \mathrm{M}\) potassium nitrate and \(155.5 \mathrm{~mL}\) of \(1.570 \mathrm{M}\) calcium nitrate are combined.
Problem 74
What volume of \(0.112 M\) ammonium sulfate contains \(5.75 \mathrm{~g}\) of ammonium ion?
Problem 75
Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?
Problem 76
Distilled water must be used in the gravimetric analysis of chlorides. Why?
Problem 77
Describe the basic steps involved in an acid-base titration. Why is this technique of great practical value?
Problem 78
How does an acid-base indicator work?
Problem 79
A student carried out two titrations using an \(\mathrm{NaOH}\) solution of unknown concentration in the burette. In one titration, she weighed out \(0.2458 \mathrm{~g}\) of KHP ([see page \(166 .]\) ) and transferred it to an Erlenmeyer flask. She then added \(20.00 \mathrm{~mL}\) of distilled water to dissolve the acid. In the other titration, she weighed out \(0.2507 \mathrm{~g}\) of KHP but added \(40.00 \mathrm{~mL}\) of distilled water to dissolve the acid. Assuming no experimental error, would she obtain the same result for the concentration of the \(\mathrm{NaOH}\) solution?
Problem 80
Would the volume of a \(0.10 \mathrm{M} \mathrm{NaOH}\) solution needed to titrate \(25.0 \mathrm{~mL}\) of a \(0.10 \mathrm{M} \mathrm{HNO}_{2}\) (a weak acid) solution be different from that needed to titrate \(25.0 \mathrm{~mL}\) of a \(0.10 \mathrm{M} \mathrm{HCl}\) (a strong acid) solution?
