Consider the mixing of 3.05 mL of 0.220 M
Mg(NO3)2 and 1.00 L of 0.180 M
K3PO4.
(a) Write a balanced chemical equation that describes the double
displacement reaction between these solutions. (Include
states-of-matter under the given conditions in your answer.)
(b) Calculate how many grams of the precipitate will form.
What would be the concentration of a solution made by diluting
46.9 mL of 4.54 M KOH to 625 mL?
1.0 mol of Cu(NO3)2 is dissolved in 1000 g of water. What is the
molality of the solution for use in colligative property equations?
The answers are 1, 2, 3, 4, or cannot be determined.
A 26.0−mL solution of 0.120 M CH3COOH is titrated with a 0.220 M
KOH solution. Calculate the pH after the following additions of the
KOH solution:
(a) 0.00 mL
(b) 5.00 mL
Find the equilibrium concentration of the Mn(C2O4)2− ion(in M)
when 0.50 L of 0.030 M Mn(NO3)2 are mixed with 1.0 L of 1.2M
Na2C2O4. Kf of Mn(C2O4)2 2- is 6.3 x 10 5.
a) Does a precipitate form when 0.200 L of 0.15 M
Ca(NO3)2 is mixed with 0.100 L of 0.120 M
NaF? At experimental temperature, Ksp of CaF2
= 3.9 x 10-11
b) Calcium hydroxide, Ca(OH)2, is an important
component of many mortars, plasters and cements. Calculate the
molar solubility of Ca(OH)2 in water if Ksp
is 6.5 x 10-6.
c) What is the solubility of Ca(OH)2 in a 0.20 M
solution of Ca(NO3)2? Ksp of
Ca(OH)2 is 6.5 x 10-6
The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5
M Al(NO3)3. What is the concentration of aluminum ions
after the aluminum nitrate has reacted with the potassium
hydroxide? Kf = 3.0 ´ 1033 for Al(OH)4– Answer:
1*10^(-31). Please explain the process thoroughly.
The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5
M Al(NO3)3. What is the concentration of aluminum ions
after the aluminum nitrate has reacted with the potassium
hydroxide? Kf = 3.0 ´ 1033 for Al(OH)4– Answer:
1*10^(-31). Please explain the process thoroughly.