10B 2 Concentration of ions in mixed solutions
Type the numerical answers to these questions to 2 significant figures (no units required).
To enter 1.23 x 10-4 simply type 1.23 x 10-4.
5.0 mL of 0.0050 mol L
-1 H
2SO
4 are added to 30.0 mL of 0.010 mol L
-1 Ca(NO
3)
2 solution.
Find [Ca2+].
5.0 mL of 0.0050 mol L
-1 H
2SO
4 are added to 30.0 mL of 0.010 mol L
-1 Ca(NO
3)
2 solution.
Find [SO42-].
Will a precipitate form if [Ca2+] = 8.6 x 10-3 mol L-1 and [SO42-] = 7.1 x 10-4 mol L-1. Ks(CaSO4) = 2 x 10-5.
- Yes
- No
3.0 mL of 0.010 mol L
-1 ZnSO
4 are added to 20.0 mL of 0.0050 mol L
-1 NaOH solution.
Find [OH-].
3.0 mL of 0.010 mol L
-1 ZnSO
4 are added to 20.0 mL of 0.0050 mol L
-1 NaOH solution.
Calculate [Zn2+].
Will a precipitate of Zn(OH)2 form if [Zn2+] = 1.3 x 10-3 mol L-1 and [OH-] = 4.3 x 10-3 mol L-1? Ks = 3 x 10-17.
- Yes
- No
0.10 mL of 0.010 mol L-1 AgNO3 solution is added to 40.0 mL of 0.0025 mol L-1 MgCl2 solution.
What is [Ag+]?
0.10 mL of 0.010 mol L
-1 AgNO
3 solution is added to 40.0 mL of 0.0025 mol L
-1 MgCl
2 solution.
What is [Cl-]?
Will a precipitate form if [Ag+] = 2.5 x 10-5 mol L-1 and [Cl-] = 5.0 x 10-3 mol L-1? Ks(AgCl) = 2 x 10-10.
- Yes
- No