1.Nitric acid is usually purchased in concentrated form with a 70.3% HNO3 concentration by mass and a density of 1.41 g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5 L of 0.500 M HNO3?
2. Complete the table.
[H3O+] [OH-] pOH pH Acid or Basic
1.0 * 10-8 1.0 * 10-6 6.00 8.00 basic
______ ______ ______ 3.55 ______
1.7 * 10-9 ______ ______ ______ ______
______ ______ ______ 13.5 ______
______ 8.6 * 10-11 ______ ______ ______
3. Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.
Compound [Cation] [Anion] Ksp
CdS 3.7 * 10-15 3.7 * 10-15 ______
BaF2 ______ 7.2 * 10-3 1.9 * 10-7
Ag2SO4 2.8 * 10-2 ______ 1.1 * 10-5
4. Coal can be used to generate hydrogen gas (a potential fuel) by this endothermic reaction.
If this reaction mixture is at equilibrium, predict the effect (shift right, shift left, or no effect) of
(a) adding more C to the reaction mixture.
(b) adding more H2O(g) to the reaction mixture.
(c) raising the temperature of the reaction mixture.
(d) increasing the volume of the reaction mixture.
(e) adding a catalyst to the reaction mixture.
5. Determine whether or not each reaction is a redox reaction. For those reactions that are redox reactions,
identify the substance being oxidized and the substance being reduced.
(a) Zn(s) + CoCl2 (aq)¡ZnCl2 (aq) + Co(s)
(b) HI(aq) + NaOH(aq)¡H2 O(l) + NaI(aq)
(c) AgNO3 (aq) + NaCl(aq)¡
AgCl(s) + NaNO3 (aq)
(d) 2 K(s) + Br2 (l)¡2 KBr(s)
6. Consider the unbalanced redox reaction:
Cr2 O72-(aq) + Cu(s)¡Cr3+(aq) + Cu2+
Balance the equation in acidic solution and determine
how much of a 0.850 M K2 Cr2 O7 solution is required to completely dissolve 5.25 g of Cu.
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