Explanation a) The K sp value of compound is 1.16 × 10 − 10 M Molar solubility = 1.08 × 10 − 5 BaCrO 4 = Ba 2 + + CrO 4 2 − K sp = [ Ba 2 + ] + [ CrO 4 2 − ] K sp = ( s ) ( s ) K sp = s 2 K sp = ( 1.08 × 10 − 5 ) 2 = 1.16 × 10 − 10 M b) The K sp value of compound is 1.48 × 10 − 14 Molar solubility = 1.55 × 10 − 5 Ag 2 SO 3 ( s ) = Ag + 2 + SO 3 2 − K sp = [ Ag + ] 2 [ SO 3 − 2 ] K sp = ( 2 s ) 2 ( s ) K sp = ( 2 × 1...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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Chapter 17, Problem 88E

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To determine:

To calculate the K_sp value of each compound in pure water by using the given molar solubility

$\begin{array}{l} (a) {BaCrO}_{4} (1.08 \times 10^{- 5}) \\ (b) {Ag}_{2} {SO}_{3} (1.55 \times 10^{- 5}) \\ (c) Pd {(SCN)}_{2} (2.22 \times 10^{- 8}) \end{array}$

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Chapter 17, Problem 87E

Chapter 17, Problem 89E

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To calculate the K sp value of each compound in pure water by using the given molar solubility ( a ) BaCrO 4 ( 1.08 × 10 − 5 ) ( b ) Ag 2 SO 3 ( 1.55 × 10 − 5 ) ( c ) Pd ( SCN ) 2 ( 2.22 × 10 − 8 )

Solution Summary: The author explains how to calculate the K sp value of each compound in pure water by using the given molar solubility.

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To determine:

To calculate the K_sp value of each compound in pure water by using the given molar solubility

$\begin{array}{l} (a) {BaCrO}_{4} (1.08 \times 10^{- 5}) \\ (b) {Ag}_{2} {SO}_{3} (1.55 \times 10^{- 5}) \\ (c) Pd {(SCN)}_{2} (2.22 \times 10^{- 8}) \end{array}$

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Chapter 17 Solutions

To calculate the K sp value of each compound in pure water by using the given molar solubility ( a ) BaCrO 4 ( 1.08 × 10 − 5 ) ( b ) Ag 2 SO 3 ( 1.55 × 10 − 5 ) ( c ) Pd ( SCN ) 2 ( 2.22 × 10 − 8 )

Solution Summary: The author explains how to calculate the K sp value of each compound in pure water by using the given molar solubility.

Concept explainers

Videos

To determine: To calculate the Ksp value of each compound in pure water by using the given molar solubility (a)BaCrO4(1.08×10−5)(b)Ag2SO3(1.55×10−5)(c)Pd(SCN)2(2.22×10−8)

Want to see the full answer?

Chapter 17 Solutions

To determine:

To calculate the K_sp value of each compound in pure water by using the given molar solubility

$\begin{array}{l} (a) {BaCrO}_{4} (1.08 \times 10^{- 5}) \\ (b) {Ag}_{2} {SO}_{3} (1.55 \times 10^{- 5}) \\ (c) Pd {(SCN)}_{2} (2.22 \times 10^{- 8}) \end{array}$