Question
In: Chemistry
1. Calculate the pH of a solution prepared by mixing 2.50 L of 2.35 M HF...
1. Calculate the pH of a solution prepared by mixing 2.50 L of 2.35 M HF with 4.50 L of 1.56 M NaF.
2. A 4.00-g sample of NaOH is added to 2.00 L of the solution prepared in problem 1. Calculate the pH of the new solution. Assume any volume change is negligible.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
Calculate the pH of a solution prepared by mixing 300mL of 0.250 m aqueous HF (dens=1.10g/mL)...
Calculate the pH of a solution prepared by mixing 300mL of 0.250 m
aqueous HF (dens=1.10g/mL) with 43.6g of an aqueous solution that
is 3.6% NaOH by mass. (dens=1.02g/mL).
Calculate the pH of a solution that is made by mixing 0.80 L of 0.30 M...
Calculate the pH of a solution that is made by mixing 0.80 L of
0.30 M formic acid (HCOOH, Ka=1.77X10-4) and 0.90 L of 0.20 M
sodium formate (NaHCOO). [Hint: don’t forget that you are mixing,
and so each is diluted upon mixing]
11. Calculate the pH of a solution prepared by mixing a) 48.0 mL of 0.212 M...
11. Calculate the pH of a solution prepared by mixing
a) 48.0 mL of 0.212 M NaOH and 66.0 mL of 0.187 M HCl
b) 69.0 mL of 0.345 M KOH and 125 mL of 0.400 M HC3H5O2
c) 350 mL of 0.130 M NH3 and 400 mL of 0.100 M HCl
Calculate the pH of a solution prepared by mixing a) 25.0 mL of 0.512 M NaOH...
Calculate the pH of a solution prepared by mixing a) 25.0 mL of
0.512 M NaOH and 34.0 mL of 0.187 M HCl b) 46.0 mL of 0.235 M KOH
and 50.0 mL of 0.420 M HC3H5O2 c) 400 mL of 0.250 M NH3 and 250 mL
of 0.120 M HCl
Calculate the pH of a solution prepared by mixing a) 25.0 mL of 0.512 M NaOH...
Calculate the pH of a solution prepared by mixing
a) 25.0 mL of 0.512 M NaOH and 34.0 mL of 0.187 M HCl
b) 46.0 mL of 0.235 M KOH and 50.0 mL of 0.420 M
HC3H5O2
c) 400 mL of 0.250 M NH3 and 250 mL of 0.120 M
HCl
Question 6 Calculate the pH of a solution prepared by mixing equal volumes of 0.050 M...
Question 6
Calculate the pH of a solution prepared by mixing equal volumes
of 0.050 M sodium oxalate, Na2C2O4 (aq), and 0.010 M
ammonium chloride, NH4Cl (aq).
For ammonium, Ka = 5.70 × 10–10; for oxalic acid,
Ka,1 = 5.60 × 10–2and Ka,2 = 5.42 × 10–5.
Hint #1: Use the charge balance
equation as your main equation. Use the mass balance and
equilibrium equations to find an expression for each species in
terms of [H3O+] or [OH–], then substitute...
Calculate the pH of a solution prepared by mixing 20 ml of 9.12 mol/L salicylic acid...
Calculate the pH of a solution prepared by mixing 20 ml of 9.12
mol/L salicylic acid with 20 ml water
1. Calculate the pH of a solution that is made by mixing 0.80 L of 0.30...
1. Calculate the pH of a solution that is made by mixing 0.80 L
of 0.30 M formic acid (HCOOH) and 0.90 L of 0.20 M sodium formate
(NaHCOO). Assume volumes are additive. (Ka, HCOOH = 1.77 * 10^-4
)
2. A 200.0 mL solution of 0.40 M ammonium chloride was titrated
with 0.80M sodium hydroxide. What was the pH of the solution after
50.0 mL of the NaOH solution were added? The Kb of ammonia is 1.76
* 10^-5...
1) Use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution prepared by mixing...
1) Use the Henderson-Hasselbalch equation to calculate the pH of
a buffer solution prepared by mixing equal volumes of 0.230 M
NaHCO3 and 9.00×10−2 M Na2CO3. (use Ka values given on
Wiki)
2) A volume of 100 mL of a 0.440 M HNO3 solution is
titrated with 0.440 M KOH. Calculate the volume of KOH
required to reach the equivalence point.
Calculate the pH of a .003 M solution of NaF, given that the Ka of HF...
Calculate the pH of a .003 M solution of NaF, given that the Ka
of HF = 6.8 x 10^-4 at 25 degrees celcius.
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