Calculate the change in pH for each buffer upon the addition of 10 mL of 1.00MHC

Question

Calculate the change in pH for each buffer upon the addition of 10 mL of 1.00MHCI. Express your answers using two decimal places. Enter your answers separated by a comma. Delta pHA, Delta pHB= Consider two buffers being prepared by adding an equal number of moles of formic acid (HCOOH) and sodium format (HCOONa) to enough water to make 1.00 L of solution. Buffer, A is prepared using 1.00 mol each of formic acid and sodium format. Buffer B is prepared by using 0.010 mol of each. Part A Calculate the pH of each buffer. Express your answers using two decimal places. Enter your answers separated by a comma. PHA,PHB= Try Again; 2 attempts remaining

Explanation / Answer

A)pHa=pka+log(salt/acid)

=pKa

=3.77

pHb=pKa+log(salt/acid)

=pKa

=3.77

D)intial pH=3.77

for A,

final pH=3.77+log((1-0.01)/(1+0.01))

=3.76

so change= -0.01

for B,

whole of the salt is converted to acid.so,

concentration of the acid=0.02

so let the dissociation be x.so,

10^(-3.77)=x^2/(0.02-x)

or x=0.00176

so pH=2.754

so change= -1.106

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.