A. How many mL of a 0.171 M aqueous solution of nickel(II) nitrate, Ni(NO3)2, must be taken to obtain 13.1 grams of the salt?
B. How many milliliters of 9.95 M hydrochloric acid solution should be used to prepare 4.00 L of 0.300 M HCl?
C. Calculate the number of milliters of 0.764 M NaOH required to precipitate as AgOH all of the Ag+ ions in 167 mL of 0.632M AgNO3 solution.
D. An aqueous solution of hydrobromic acid is standardized by titration with a 0.169 M solution of barium hydroxide.
If 13.0 mL of base are required to neutralize 13.0 mL of the acid, what is the molarity of the hydrobromic acid solution?
E. Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula is H2C2O4•2H2O.
A student dissolves 0.631 grams of H2C2O4•2H2O in water and titrates the resulting solution with a solution of sodium hydroxide of unknown concentration. If 24.1 mL of the sodium hydroxide solution are required to neutralize the acid, what is the molarity of the sodium hydroxide solution ?
F. The concentration of Cu+ in a solution is determined by titrating it with a 0.1665 M permanganate solution. The balanced net ionic equation for the reaction is:
MnO4-(aq)
- +
5Cu+(aq)+8H3O+(aq)Mn2+(aq)
- +
5Cu2+(aq)+12H2O(l)
In one experiment, 24.58 mL of the 0.1665 M permanganate solution is required to react completely with 20.00 mL of the Cu+ solution. Calculate the concentration of the Cu+ solution.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
