GENERAL,ORGANIC,+BIOCHEMISTRY
GENERAL,ORGANIC,+BIOCHEMISTRY
10th Edition
ISBN: 9781260148954
Author: Denniston
Publisher: RENT MCG
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Chapter 8, Problem 8.71QP

(a)

Interpretation Introduction

Interpretation:

The concentration of hydronium ion and hydroxide ion of a urine sample with pH=6.00 have to be calculated.

Concept Introduction:

pH:  The pH of a solution is defined as the negative logarithm of the molar concentration of the hydronium ion.

    pH=-log[H3O+]

(a)

Expert Solution
Check Mark

Explanation of Solution

Given,

    pH=6.00

The concentration of hydronium ion and hydroxide ion of a urine sample are calculated as,

    pH=6.00pH=-log[H3O+][H3O+] = 10-pH[H3O+] = 10-6.00=1×10-6M[H3O+][OH-]=1×10-14[OH-]=1×10-141×10-6=1×10-8M.

(b)

Interpretation Introduction

Interpretation:

The concentration of hydronium ion and hydroxide ion of a urine sample with pH=5.20 have to be calculated.

Concept Introduction:

Refer to part a

(b)

Expert Solution
Check Mark

Explanation of Solution

Given,

    pH=5.20

The concentration of hydronium ion and hydroxide ion of urine sample are calculated as,

    pH=5.20pH=-log[H3O+][H3O+] = 10-pH[H3O+] = 10-5.20=6.31×10-6M[H3O+][OH-]=1×10-14[OH-]=1×10-146.31×10-6=1.58×10-9M.

(c)

Interpretation Introduction

Interpretation:

The concentration of hydronium ion and hydroxide ion of a urine sample with pH=7.80 have to be calculated.

Concept Introduction:

Refer to part a

(c)

Expert Solution
Check Mark

Explanation of Solution

Given,

    pH=7.80

The concentration of hydronium ion and hydroxide ion of urine sample are calculated as,

    pH=7.80pH=-log[H3O+][H3O+] = 10-pH[H3O+] = 10-7.80=1.58×10-8M[H3O+][OH-]=1×10-14[OH-]=1×10-141.58×10-8=6.33×10-7M.

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Chapter 8 Solutions

GENERAL,ORGANIC,+BIOCHEMISTRY

Ch. 8.1 - The hydroxide ion concentration in a sample of...Ch. 8.2 - Calculate the pH of a 1.0 × 10−4 M solution of...Ch. 8.2 - Calculate the [H3O+] of a solution of HNO3 that...Ch. 8.2 - Calculate the pH corresponding to a 1.0 × 10−2 M...Ch. 8.2 - Calculate the [H3O+] and [OH−] of a potassium...Ch. 8.2 - Calculate the [H3O+] corresponding to pH =...Ch. 8.2 - Prob. 8.9PPCh. 8.2 - Calculate the [OH–] of a 1.0 × 10–3 M solution of...Ch. 8.2 - Prob. 8.10QCh. 8.3 - Calculate the molar concentration of a sodium...Ch. 8.4 - A buffer solution is prepared in such a way that...Ch. 8.4 - Prob. 8.12PPCh. 8.4 - Prob. 8.11QCh. 8.4 - Prob. 8.12QCh. 8.4 - Prob. 8.13QCh. 8.4 - Prob. 8.14QCh. 8.4 - Prob. 8.15QCh. 8.4 - Prob. 8.16QCh. 8.4 - Prob. 8.17QCh. 8.4 - Explain how the pH of blood would change under...Ch. 8.4 - Write the Henderson-Hasselbalch expression for the...Ch. 8.4 - Prob. 8.20QCh. 8.5 - Prob. 8.21QCh. 8.5 - Prob. 8.22QCh. 8.5 - Prob. 8.23QCh. 8.5 - Prob. 8.24QCh. 8.5 - Chrome plating involves the reduction of Cr3+(aq)...Ch. 8.5 - Prob. 8.26QCh. 8 - Prob. 8.27QPCh. 8 - Define a base according to the Arrhenius...Ch. 8 - What are the essential differences between the...Ch. 8 - Why is ammonia described as a Brønsted-Lowry base...Ch. 8 - Classify each of the following as either a...Ch. 8 - Classify each of the following as either a...Ch. 8 - Classify each of the following as either a...Ch. 8 - Classify each of the following as either a...Ch. 8 - Write an equation for the reaction of each of the...Ch. 8 - Write an equation for the reaction of each of the...Ch. 8 - Write the formula of the conjugate acid of CN−. Ch. 8 - Write the formula of the conjugate acid of Br−. Ch. 8 - Write the formula of the conjugate base of HI. Ch. 8 - Write the formula of the conjugate base of HCOOH. Ch. 8 - Write the formula of the conjugate acid of NO3−. Ch. 8 - Write the formula of the conjugate acid of F−. Ch. 8 - Which is the stronger base, NO3− or CN−? Ch. 8 - Prob. 8.44QPCh. 8 - Prob. 8.45QPCh. 8 - Which is the stronger base, F− or CH3COO−? Ch. 8 - Identify the conjugate acid-base pairs in each of...Ch. 8 - Identify the conjugate acid-base pairs in each of...Ch. 8 - Distinguish between the terms acid-base strength...Ch. 8 - Label each of the following as a strong or weak...Ch. 8 - Label each of the following as a strong or weak...Ch. 8 - Calculate the [H3O+] of an aqueous solution that...Ch. 8 - Calculate the [H3O+] of an aqueous solution that...Ch. 8 - Calculate the [OH−] of an aqueous solution that...Ch. 8 - Prob. 8.56QPCh. 8 - Prob. 8.57QPCh. 8 - What is the concentration of hydronium ions in an...Ch. 8 - Prob. 8.59QPCh. 8 - Consider two beakers, one containing 0.10 M NaOH...Ch. 8 - Calculate the pH of a solution that is: 1.0 × 10−2...Ch. 8 - Calculate the pH of a solution that is: 1.0 × 10−1...Ch. 8 - Calculate [H3O+] for a solution of nitric acid for...Ch. 8 - Calculate [H3O+] for a solution of hydrochloric...Ch. 8 - Prob. 8.65QPCh. 8 - Prob. 8.66QPCh. 8 - Calculate both [H3O+] and [OH−] for a solution for...Ch. 8 - Calculate both [H3O+] and [OH−] for a solution for...Ch. 8 - What is a neutralization reaction? Ch. 8 - Describe the purpose of a titration. Ch. 8 - Prob. 8.71QPCh. 8 - The pH of urine may vary between 4.5 and 8.2....Ch. 8 - Criticize the following statement: A lakewater...Ch. 8 - Can a dilute solution of a strong acid ever have a...Ch. 8 - What is the H3O+ concentration of a solution with...Ch. 8 - What is the H3O+ concentration of a solution with...Ch. 8 - Prob. 8.77QPCh. 8 - Prob. 8.78QPCh. 8 - Calculate the pH of a solution that has [H3O+] =...Ch. 8 - Calculate the pH of a solution that has [H3O+] =...Ch. 8 - Calculate the pH of a solution that has [OH−] =...Ch. 8 - Calculate the pH of a solution that has [OH−] =...Ch. 8 - Prob. 8.83QPCh. 8 - Prob. 8.84QPCh. 8 - Prob. 8.85QPCh. 8 - Prob. 8.86QPCh. 8 - Write an equation to represent the neutralization...Ch. 8 - Write an equation to represent the neutralization...Ch. 8 - Prob. 8.89QPCh. 8 - Prob. 8.90QPCh. 8 - Prob. 8.91QPCh. 8 - Prob. 8.92QPCh. 8 - Titration of 15.00 mL of HCl solution requires...Ch. 8 - Titration of 17.85 mL of HNO3 solution requires...Ch. 8 - Prob. 8.95QPCh. 8 - Prob. 8.96QPCh. 8 - Prob. 8.97QPCh. 8 - Prob. 8.98QPCh. 8 - Which of the following are capable of forming a...Ch. 8 - Which of the following are capable of forming a...Ch. 8 - Prob. 8.101QPCh. 8 - Prob. 8.102QPCh. 8 - Prob. 8.103QPCh. 8 - Prob. 8.104QPCh. 8 - For the equilibrium situation involving acetic...Ch. 8 - Prob. 8.106QPCh. 8 - Prob. 8.107QPCh. 8 - Prob. 8.108QPCh. 8 - Prob. 8.109QPCh. 8 - For the buffer system described in Question 8.105,...Ch. 8 - Prob. 8.111QPCh. 8 - Prob. 8.112QPCh. 8 - Prob. 8.113QPCh. 8 - Prob. 8.114QPCh. 8 - Prob. 8.115QPCh. 8 - Prob. 8.116QPCh. 8 - Prob. 8.117QPCh. 8 - Prob. 8.118QPCh. 8 - In the following reaction, identify the oxidized...Ch. 8 - Prob. 8.120QPCh. 8 - Prob. 8.121QPCh. 8 - Prob. 8.122QPCh. 8 - Prob. 8.123QPCh. 8 - Prob. 8.124QPCh. 8 - Prob. 8.125QPCh. 8 - Prob. 8.126QPCh. 8 - Prob. 1MCPCh. 8 - Prob. 2MCPCh. 8 - Prob. 3MCPCh. 8 - Prob. 4MCPCh. 8 - Prob. 5MCP
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