Calculate the hydrogen ion concentration and the pH of the solution
formed when 0.020 gram-formula weight of nitric acid is added to one
liter of aqueous 0.20 M ammonia solution. Assume no significant volume
change upon addition of the acid.
Calculate the molar concentration of acetic acid at equilibrium in an
acetic acid solution that is 1.1% ionized.
Given a pure 0.50 M of HCN solution, calculate the volume that when
diluted to a total volume of 70.0mL will yield a pH that is 0.65 unit
higher than that of the given solution. Consider the volumes of the
original solution and of the diluent to be precisely additive.
Calculate the pH of 0.0013 M of NaCN.
Calculate the pH of a solution which is 0.092 M in acetic acid and 0.092
M in sodium acetate.
Calculate the pH of a mixture of 50mL of 0.10 M ammonium hydroxide and
51mL of 0.10 M of HCl.
The solubility of ZnS is 3.5 x 10^-12 at 25 degrees Celsius.
Calculate the value of K for ZnS at this temperature.
sp
8) Calculate the solubility of magnesium hydroxide at 25 degrees
Celsius in (a) pure water and (b) a solution having a pH = 12.00. K
for Mg(OH) is 8.9 x 10^-12 at this temperature.
sp 2
9) The value of the solubility product of lead chloride, PbCl ,is 1.6
x 10^-5 at 25 degrees Celsius.
2
5.0 mL of 0.02 M Pb(NO ) is mixed with 25 mL of 0.01M of HCl. Does
PbCl precipitate? 3 2
2
Chemistry Homework Solutions
#44259
Taking chem class in summer term fast pace need help to pass.
I have posted these once before but, some of the material is different in my chem II book. The teacher will give us a mid-term and a final in class so, these take homes are a opportunity to get good scores to pass the class. If you accept this post would you please include equations and answers so I can practice setting up the equation and working back to the answer. Thank You.
1) Calculate the hydrogen ion concentration and the pH of the solution formed when 0.020 gram-formula weight of nitric acid is added to one liter of aqueous 0.20 M ammonia solution. Assume no significant volume change upon addition of the acid.
2) Calculate the molar concentration of acetic acid at equilibrium in an acetic acid solution that is 1.1% ionized.
3) Given a pure 0.50 M of HCN solution, calculate the volume that when diluted to a total volume of 70.0mL will yield a pH that is 0.65 unit higher than that of the given solution. Consider the volumes of the original solution and of the diluent to be precisely additive.
4) Calculate the pH of 0.0013 M of NaCN.
5) Calculate the pH of a solution which is 0.092 M in acetic acid and 0.092 M in sodium acetate.
6) Calculate the pH of a mixture of 50mL of 0.10 M ammonium hydroxide and 51mL of 0.10 M of HCl.
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