Design a buffer that has a pH of 10.00 using one of the weak base/conjugate acid systems shownbelow.Weak BaseConjugate AcidKapK.CH3NH,4.2x104 CH3NH3"2.4x10-11 10.62C,H1503N 5.9x107 C,H1503NH*1.7×10-87.77C3H;N1.5×109 C3H;NH*6.7×10-65.17How many grams of the chloride salt of the conjugate acid must be combined with how many gramsof the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams chloride salt of conjugate acid =grams weak base =

Given, pH of the buffer = 10.00 Volume of the buffer = 1.00 L [Weak base] = [CH3NH2] = 1.00 M…

Design a buffer that has a pH of 10.00 using one of the weak base/conjugate acid systems shown below. Weak Base Kp Conjugate Acid Ka pKa CH3NH2 4.2x104 CH3NH3 2.4×10-11 10.62 C,H1503N 5.9×10-7 | C,H1503NH* 1.7×10-8 7.77 C3H;N 1.5×10° C3H3NH* 6.7×10-6 5.17 How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =|

Design a buffer that has a pH of 10.00 using one of the weak base/conjugate acid systems shown below. Weak Base Kp Conjugate Acid Ka pKa CH3NH2 4.2x104 CH3NH3 2.4×10-11 10.62 C,H1503N 5.9×10-7 | C,H1503NH* 1.7×10-8 7.77 C3H;N 1.5×10° C3H3NH* 6.7×10-6 5.17 How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =|

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...

See similar textbooks

Similar questions

A student needs to prepare a buffer solution with a pH of 4.54. Assuming a pKg of 4.58, how many ml of 0.1 M NAOH would need to be added to 20.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pK, + log ([B minus]/[HB]) or, if concentrations are the same, pH = pk, + log (Volume of OH minus/ (Volume of HB minus Volume of OH minus)
What is the pH of a solution created by mixing 25.00 mL of 0.10 M formic acid and 25.00 mL of 0.10 M sodium format? Ka of formic acid is 1.8 X 10-4 -1.8 X 10-4 -3.74 -4.74 -1.00
An acetate buffer has a ph of 5, how much will be ionized? how much will be unionized? how much of drug P (kb = 7 x 10^-8) in solution at pH 8 will be: ionized? unionized?
Calculate the pH of a buffer solution prepared by dissolving .37 moles of formic acid (HCO2H) and .23 moles of sodium formate (NaCO2H) in 1.00 L of solution. (Ka = 1.8 x 10-4 ) Group of answer choices 2.09 2.30 10.46 3.54
Complete solution
01 5 If the dissociation constant of a weak acid is 8.1 x 10-5, at what ratio should you adjust the concentration of the weak acid and its conjugate base in order that has a pH of 4.09? prepare a buffer Oa) 0.100 M veak acid with 0.100 M conjugate base b) 0.100 M weak acid with 0.0100 M conjugate base Oc) 0.100 M weak acid with 0.0500 M conjugate base d) 1.000 M weak acid with 0.0100 M conjugate base e) 0.510 M weak acid with 0.0510 M conjugate base 0 000 О
Which of the following would have the highest buffer capacity? Group of answer choices 1.0 M HCN / 1.0 M CN- 0.500 M NH4+ / 0.500 M NH3 0.40 M HF / 0.40 M F- 0.35 M HCOOH / 0.35M HCOO- 0.25 M HCO3- / 0.25 M CO32-
Give a clear handwritten answer with explanation
Calculate the pH of each of the following buffered solutions. Ka of acetic acid = 1.8 x 10-5, Kb of C2H5NH2 = 5.6 x 10-4 a)0.10 M acetic acid and 0.25 M sodium acetate b)0.25 M acetic acid and 0.10 M sodium acetate c)0.25 M acetic acid and 0.25 M sodium acetate d)0.50 M C2H5NH2 and 0.25 M C2H5NH3Cl e)0.50 M C2H5NH2 and 0.50 M C2H5NH3
Design a buffer that has a pH of 4.66 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 × 10-5 4.19 H2PO4- HPO42- 6.2 × 10-8 7.21 HCO3- CO32- 4.8 × 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams potassium salt of weak acid = grams potassium salt of conjugate base =
Which of the following will give a buffer with a pH near 4.76 when the acid and conjugate base are mixed in equimolar proportions? Acid NH4* (from ammonia) HC₂H3O2 (acetic acid) HF (hydrofluoric acid) CH3CH₂NH3 (from ethylamine) acetic acid. b) ethylamine c) ammonia d) hydrofluoric acid e) none Ka 5.69 10-10 1.75 10-5 6.810-4 2.12 10-11
Pp