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Chapter 10: Q. 10.61 (page 354)

Someone with kidney failure excretes urine with large amounts ofHCO3-. How would this loss of HCO3-affect the pHof the blood plasma?

Short Answer

Expert verified

WhenHCO3- excreted in urine, it rises to a higher level.

So the blood pressure of pHdrops.

Step by step solution

01

Step - 1   Introduction

  • Text Carbonic acid interacts with water to produce the hydronium ion and HCO3-text.
  • The following is the reaction:

H2CO3+H2O(l)鈬�HCO3-+H3O+

02

Step - 2  Explanation

  • When more HCO3-is excreted by urine, the equilibrium moves to a higher H3O+.
  • The bloodpH drops as a result of this.

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Most popular questions from this chapter

Identify the Bronsted-Lowry acid-base pairs in each of the following equations:

a.H3PO4(aq)+H2O(l)鈬�H2PO4-(aq)+H3O+(aq)

b.localid="1652710222540" CO3(2-aq)+H2O(l)鈬�HCO3-(aq)+OH-(aq)

c.localid="1652710226359" H3PO4(aq)+NH3(aq)鈬�H2PO4-(aq)+NH4+(aq)

For each of the following: (10.2,10.3)

1. H2S 2.H3PO4

a. Write the formula for the conjugate base.

b. Which is the weaker acid?

If 32.8mLof a 0.162MNaOHsolution is required to titrate 25.0mLof a solution of H2SO4, what is the molarity of the H2SO4solution?

H2SO4(aq)+2KOH(aq)鉄�2H2O(l)+K2SO4(aq)

A buffer solution is made by dissolving H3PO4andNaH2PO4in water(10.8)

A. Write an equation that shows how this buffer neutralizes added acid.

B. Write an equation that shows how this buffer neutralizes added base.

Consider the buffer system of hydrofluoric acid, HF, and its salt, NaF .

HF(aq)+H2O(l)鈬�H3O+(aq)+F-(aq)

a. The purpose of this buffer system is to:

1. maintain [HF]

2. maintain F-

3. maintain pH

b. The salt of the weak acid is needed to:

1. provide the conjugate base

2. neutralize added H3O+

3. provide the conjugate acid

c. If OH-is added, it is neutralized by:

1. the salt

2. H2O

3. H3O+

d. WhenH3O+is added, the equilibrium shifts in the direction of the:

1. reactants

2. products

3. does not change
See all solutions

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