if 0.050 mol of hcl is added to 1.0 l of buffer solution
containing 0.125 M potassium acetate and 0.10 M acetic acid what is
the change in PH of the solution
0.2 mol of gaseous HCl is added to 1.0 L of a buffer solution
that contains 3.0 M CH3COOH and 3.0 M
CH3COONa. What is the pH of the solution? Assume that
Ka for CH3COOH is 10-5. Assume
also that the volume of the solution does not change when the HCl
is added.
Type your answer in decimal number carrying only one digit after
decimal. So you must round up or down at the second digit after
decimal.
For example,...
A 360.0 ml buffer solution is 0.130 mol/L in HF and 0.130 mol/L in NaF.
Part A : what mass of NaOH could this buffer neutralize before the PH rises above 4.00?
Part B: If the same volume of the buffer was 0.370mol/L in NaF, what mass of NaOH could be handled before the pH rises above 4.0?
the Ka of HF is 3.5*10^-4 this is all the information given, I can look up more ka or...
what mass of Ca(NO3)2 must be added to 1.0
L of a 1.0 M HF solution to begin precipitation of CaF2.
You may assume no volume change on the addition of
Ca(NO3)2. Ksp for CaF2 = 4.0 x
10-11 and ka for HF=7.2 x
10-4.
Calculate the pH after 0.14 mole of NaOH is added to 1.09 L of a
solution that is 0.49 M HNO2 and 1.18
M NaNO2, and calculate the pH after 0.28 mole
of HCl is added to 1.09 L of the same solution of HNO2
and NaNO2.
0.14 mole of
NaOH
0.28 mole of
HCl
A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.
Calculate the pH of the solution after the addition of 0.0500 moles
of solid NaOH. Assume no volume change upon the addition of base.
The Ka for HF is 3.5 × 10-4.
How many moles of HCl must be added to 1.0 L of 1.0 M NH3(aq) to
make a buffer with a pH of 9.00? (pKa of NH4+ =9.25)
the answer is 0.64, explain please.