The presence of CO32", HCO3 and CO2 in body fluids helps to stabilize the pH of these fluids despite the addition or removal of H* ions by body processes. Ka,1 and Ka,2 for H2CO3 are 4.2*10-7 and 4.7*10-11, respectively. If the "normal" pH in blood plasma is 7.40, identify the components that would provide the best buffer at this pH. Н2СОЗ and НСОЗ- Н2СОЗ, НСО3-and CO32- HCO3- and CO32- CO2 and CO32- H2CO3 and CO32-

The presence of CO32", HCO3 and CO2 in body fluids helps to stabilize the pH of these fluids despite the addition or removal of H* ions by body processes. Ka,1 and Ka,2 for H2CO3 are 4.210-7 and 4.710-11, respectively. If the "normal" pH in blood plasma is 7.40, identify the components that would provide the best buffer at this pH. Н2СОЗ and НСОЗ- Н2СОЗ, НСО3-and CO32- HCO3- and CO32- CO2 and CO32- H2CO3 and CO32-

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 350,0 mL buffer solution is 0.170 moll-1 in HF and 0.170 moll-1 in NaF. Ka(HF)=6,3x10-4 a) What mass of NaOH could this buffer neutralize before the pH rises above 4.00? Express your answer using two significant figures. b) If the same volume of the buffer was 0.350 molL-1 in HF and 0.350 molL-1 in NaF, what mass of NaOH could be handled before the pH rises above 4.00? Express your answer using two significant figures.
A buffer with a pH of 9.71 is to be prepared from NH3 and NH4Cl. What ratio of base to saltwould you use? KB(NH3)=1.8x10‒5 (give your answer to 3 sig figs)
What is the pH of a buffer solution made of .50 M CH3CO2H and .36 M NaCH3CO2? pka= 4.7 for CH3CO2H
(3) How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid (C6H8O7) [Atomic weight: C = and solid sodium citrate (Na3C6H5O7).The Ka of citric acid is 7.40 x 10-4. 12.01 amu, H = 1.00 amu, O 16.00 amu, Na 23.00 amu] man 13
1) A 1.0L solution of 1.0 M NaF is titrated with 1.0 M HCI, What is the pH of the solution after the addition of 0.00, 0.50, 1.0, and 1.5 L of 1.0 M HCI? The pk, of HF is 3.17. 2) A15L solution of 1.0x10 M HCIO, is titrated with 2.0x10 MCa(OH),. What is the pH of the solution after the addition of 0.00, 0.25, and 0.50 L of 2.0x10 M Ca(OH);? The pk, of HCIO, is 1.96.
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A chemistry graduate student is given 100. mL of a 1.70M diethylamine ((C2H5)2NH): NH solution. Diethylamine is a weak base with K = 1.3 × 10³. What mass of (C₂Hs)2NH2Br should the student dissolve in the (C2H3)2NH solution to turn it into a buffer with pH = 11.12? You may assume that the volume of the solution doesn't change when the (C2H5)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10
Be sure to answer all parts. A buffer consists of 0.30 M KHCO3 and 0.69 M K₂CO3. Carbonic acid is a diprotic acid with Kal-4.5 x 107 and K₁2 = 4.7 x 10-¹1. (a) Which K, value is more important to this buffer? Kat is more important. OK₁2 is more important. (b) What is the buffer pH?
A buffer solution is prepared in such a way that the concentration of propanoic acid is 3.9 x 10-1 power M and the concentration of sodium propanoate is 1.8 x 10 0 power M. The buffer equilibrium is described by C2H5cooH + H20 both arrows H3O+ c2h5COO- with Ka= 1.34 x 10 - 5 power . if the concentration of the sodium propanoate were double propanotate were doubled while the acide concentration remained the same, calculate the pH of the resulting solution pH = _______
What is the pH of a buffer that is 0.200M HC2H3O2 and 0.100M NaC2H3O2 (Ka =1.8 x 10-5).
How many miciolters of1.000MNaOHsolution must be added to25.00 mLof a0.1000Msolition of lactic acid(CH3CH(OH)COOHorHC3H5O2)to produce a buffer withpH=3.55? Express your answer
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2–9.3? CH3COONA / CH3COOH (Ka = 1.8 x 10-5) %D NH3 / NHẠCI (Ka = 5.6 x 10-10) NaOCI / HOCI (Ką = 3.2 x 10-8) NaNO2 / HNO2 (Ka = 4.5 × 104) %D