CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
8th Edition
ISBN: 9781305079298
Author: Masterton
Publisher: Cengage Learning
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Chapter 14, Problem 36QAP

There is a buffer system in blood H 2 PO 4 HPO 4 2 that helps keep the blood pH at 7.40. ( K a H 2 PO 4 = 6.2 × 10 8 ) .

(a) Calculate the [ H 2 PO 4 ] / [ HPO 4 2 ] ratio at the normal pH of blood.

(b) What percentage of the HPO 4 2 ions are converted to H 2 PO 4 when the pH is 7.00?

(c) What percentage of the H 2 PO 4 ions are converted to HPO 4 2 when the pH is 8.00?

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

The ratio [H2PO4][HPO42] should be determined for the blood system.

Concept introduction:

Henderson-Hasselbalch equation is an equation useful to determine the pH of any solution when any acid’s aqueous solution is related to its acid dissociation constant.

Buffer equation is considered as an equation when ionization of a weak acid in the water occurs resulted into the hydronium ion and the conjugate base of that acid.

Answer to Problem 36QAP

The ratio [H2PO4][HPO42] is 0.64 for the blood system.

Explanation of Solution

For H2PO4, we have below-mentioned dissociation equation:

H2PO4(aq)H+(aq)+HPO42(aq)

For acid-dissociation constant of the given H2PO4- is as mentioned below:

Ka=[H+][H2PO4][HPO42][H+]Ka=[H2PO4][HPO42]....(1)

For H2PO4 solution, we have Ka=6.2×108 and blood pH as 7.40.

Now, we need to determine the concentration of [H+] and we can use pH formula for the same.

pH=-log10[H+]7.40=-log10[H+][H+]=107.40[H+]=3.98×108

In equation (1), we are substituting the value of [H+] as below.

[H+]Ka=[H2PO4][HPO42][H2PO4][HPO42]=3.98×1086.2×108[H2PO4][HPO42]=0.64

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

The percentage HPO42 should be determined whichis converted into HPO42 when the pH is 6.80.

Concept introduction:

Henderson-Hasselbalch equation is an equation useful to determine the pH of any solution when any acid’s aqueous solution is related to its acid dissociation constant.

Buffer equation is considered as an equation when ionization of a weak acid in the water occurs resulted in the hydronium ion and the conjugate base of that acid.

Answer to Problem 36QAP

HPO42 ions as 54% that are converted into H2PO4 when the pH is 6.80.

Explanation of Solution

The pH of the buffer system as 6.80and the ratio of the concentration of HPO42 and H2PO4 as 0.64.

Now, let us take the concentration of H2PO4 as 1M so that we can determine the concentration of HPO42 as follow.

[H2PO4][HPO42]=0.64[HPO42]=10.64[HPO42]=1.56M

We have the dissociation equation of H2PO4 as follow:

H2PO4(aq)H+(aq)+HPO42(aq)I: 0.100          0.156C: +x             -xE: 0.100+x     0.100-x

As per the Henderson-Hasselbalch equation,

pH= pKa+ log[base][acid]pH= pKa+ log[HPO42][H2PO4]6.80= -log10(6.2×108)+log100.156x0.100+x6.80= 7.21+log100.156x0.100+xx=0.0842M

Now, the percentage of HPO42 which is converted to H2PO4 is,

0.08420.156×100=54%

Expert Solution
Check Mark
Interpretation Introduction

(c)

Interpretation:

The percentage H2PO4 should be determined which is converted into HPO42 when the pH is 7.80.

Concept introduction:

Henderson-Hasselbalch equation is an equation useful to determine the pH of any solution when any acid’s aqueous solution is related to its acid dissociation constant.

Buffer equation is considered as an equation when ionization of a weak acid in the water occurs resulted in the hydronium ion and the conjugated base of that acid.

Answer to Problem 36QAP

H2PO4 as 47% are converted into HPO42 when the pH is 7.80.

Explanation of Solution

We have the pH of the buffer system as 7.80 and the ratio of the concentration of HPO42 and H2PO4 as 0.64.

Now, let us take the concentration of H2PO4 as 1M so that we can determine the concentration of HPO42 as follow.

[H2PO4][HPO42]=0.64[HPO42]=10.64[HPO42]=1.56M

We have the dissociation equation of H2PO4 as follow:

H2PO4(aq)H+(aq)+HPO42(aq)I: 0.100          0.156C: -y             +yE: 0.100-y     0.100+y

As per the Henderson-Hasselbalch equation,

pH= pKa+ log[base][acid]pH= pKa+ log[HPO42][H2PO4]7.80= -log10(6.2×108)+log100.156+y0.100y7.80= 7.21+log100.156+y0.100yy= 0.047 M

Now, the percentage of H2PO4 which is converted to HPO42 is,

0.0471.00×100=47%

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Chapter 14 Solutions

CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS

Ch. 14 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 14 - A buffer is prepared by dissolving 0.062 mol of...Ch. 14 - A buffer solution is prepared by adding 15.00 g of...Ch. 14 - A buffer solution is prepared by adding 5.50 g of...Ch. 14 - A solution with a pH of 9.22 is prepared by adding...Ch. 14 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Consider the weak acids in Table 13.2. Which...Ch. 14 - Prob. 24QAPCh. 14 - A sodium hydrogen carbonate-sodium carbonate...Ch. 14 - You want to make a buffer with a pH of 10.00 from...Ch. 14 - Prob. 27QAPCh. 14 - The buffer capacity indicates how much OH- or H+...Ch. 14 - A buffer is made up of 0.300 L each of 0.500 M...Ch. 14 - A buffer is made up of 239 mL of 0.187 M potassium...Ch. 14 - Enough water is added to the buffer in Question 29...Ch. 14 - Enough water is added to the buffer in Question 30...Ch. 14 - A buffer is prepared in which the ratio [ H2PO4...Ch. 14 - A buffer is prepared using the butyric...Ch. 14 - Blood is buffered mainly by the HCO3 H2CO3 buffer...Ch. 14 - There is a buffer system in blood H2PO4 HPO42 that...Ch. 14 - Given three acid-base indicators—methyl orange...Ch. 14 - Given the acid-base indicators in Question 37,...Ch. 14 - Metacresol purple is an indicator that changes...Ch. 14 - Thymolphthalein is an indicator that changes from...Ch. 14 - When 25.00 mL of HNO3 are titrated with Sr(OH)2,...Ch. 14 - A solution of KOH has a pH of 13.29. It requires...Ch. 14 - A solution consisting of 25.00 g NH4Cl in 178 mL...Ch. 14 - A 50.0-mL sample of NaHSO3 is titrated with 22.94...Ch. 14 - A sample of 0.220 M triethylamine, (CH3CH2)3 N, is...Ch. 14 - A 35.00-mL sample of 0.487 M KBrO is titrated with...Ch. 14 - A 0.4000 M solution of nitric acid is used to...Ch. 14 - A 0.2481 M solution of KOH is used to titrate...Ch. 14 - Consider the titration of butyric acid (HBut) with...Ch. 14 - Morphine, C17H19O3N, is a weak base (K b =7.4107)....Ch. 14 - Consider a 10.0% (by mass) solution of...Ch. 14 - A solution is prepared by dissolving 0.350 g of...Ch. 14 - Prob. 53QAPCh. 14 - Ammonia gas is bubbled into 275 mL of water to...Ch. 14 - For an aqueous solution of acetic acid to be...Ch. 14 - Prob. 56QAPCh. 14 - Prob. 57QAPCh. 14 - Water is accidentally added to 350.00 mL of a...Ch. 14 - A solution of an unknown weak base...Ch. 14 - Consider an aqueous solution of HF. The molar heat...Ch. 14 - Each symbol in the box below represents a mole of...Ch. 14 - Use the same symbols as in Question 61 ( = anion,...Ch. 14 - The following is the titration curve for the...Ch. 14 - Prob. 64QAPCh. 14 - Follow the directions of Question 64. Consider two...Ch. 14 - Prob. 66QAPCh. 14 - Indicate whether each of the following statements...Ch. 14 - Prob. 68QAPCh. 14 - Consider the following titration curves. The...Ch. 14 - Consider the titration of HF (K a=6.7104) with...Ch. 14 - The species called glacial acetic acid is 98%...Ch. 14 - Four grams of a monoprotic weak acid are dissolved...Ch. 14 - Prob. 73QAPCh. 14 - Fifty cm3 of 1.000 M nitrous acid is titrated with...Ch. 14 - A diprotic acid, H2B(MM=126g/moL), is determined...Ch. 14 - Prob. 76QAPCh. 14 - Two students were asked to determine the Kb of an...Ch. 14 - How many grams of NaOH must be added to 1.00 L of...Ch. 14 - How many grams of NaF must be added to 70.00 mL of...Ch. 14 - Prob. 80QAP
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