Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Write K expression for the following reaction:
2H2O2(aq) ↔ 2H2O(l) + O2(g)
Consider the following reaction:
Ag+ (ag) + 2 NH3 (aq) = Ag(NH3)2+ (aq) Keq = 7.99
An initial concentration of Ag+ = 0.0100 M was combined with NH3 and allowed to reach equilibrium. If the equilibrium concentration of Ag(NH3)2+= 0.00278 M, What was the initial concentration of NH3?
Cu2+(aq) + H2O(l) ⇌ CuOH+(aq) + H+(aq) Keq = 1.2 x 10−8
A 1.00 M solution of copper(II) nitrate is created and the system shown above reaches equilibrium. What happens to the pH of the system if more CuOH+ is added after reaching equilibrium?
The pH of the system will not change because of the small size of K.
The pH of the system will increase because of the increased concentration of CuOH+.
The pH of the system will increase as the reverse reaction proceeds at a faster rate to reestablish equilibrium.
The pH of the system will decrease as the forward reaction proceeds at a faster rate to reestablish equilibrium.
Chapter 16 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 16 - Prob. 16.2VPCh. 16 - Prob. 16.3VPCh. 16 - Prob. 16.4VPCh. 16 - Prob. 16.5VPCh. 16 - Prob. 16.6VPCh. 16 - Prob. 16.7VPCh. 16 - Prob. 16.8VPCh. 16 - Prob. 16.9VPCh. 16 - Prob. 16.10VPCh. 16 - Prob. 16.11QA
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- Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.arrow_forwardFill in the left side of this equilibrium constant equation for the reaction of dimethylamine ((CH,) NH), a weak base, with water. (CH), ロ回 | = K,arrow_forwardA solution is prepared by adding 4.53 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO3)2. The equilibrium concentration of cobalt ions can be expressed with the scientific notation: [Co^2+] = a x 10^-9M. What is the value of coefficient a? Report one decimal place. Kf= 5.0 x 10^9 for Co(OH)4^2-arrow_forward
- Given that K(eq) = K(sp), calculate concentration of the aqueous cation formed at equilibrium when excess solid FeS is placed in water if K(eq) = 8.00 × 10⁻¹⁹.arrow_forwardWrite the general equilibrium constant for 2 NaBr(aq) + Pb(ClO4)2(aq) → PbBr2(s) + 2 NaClO4(aq). K = 1 / [Pb^2+][Br^−] 2 K = [NaClO4]^2 / [NaBr]^2 [Pb(ClO4)2] K = [Pb^2+][Br−]^2 K = [PbBr2] / [Pb^2+][Br−]^2 K = 1 / [Pb(ClO4)2][NaBr]^2arrow_forwardWhat are the equilibrium concentrations when 0.25 mol Ni2+ is added to 1.00 L of 2.00 M NH3 solution? Ni2+(aq) + 6NH3(aq) ⇌ Ni(NH3)6 2+(aq) Kc = 5.5 × 108With such a large equilibrium constant, first form as much product as possible, then assume that only a small amount (x) of the product shifts left. Calculate the error in your assumption.arrow_forward
- Complete the following solubility constant expression for Co(OH)2. K = sp X Śarrow_forwardammonium chloride decomposes according to the equation: NH4CI -> NH3 + HCL. Calculate the number of g of NH4C16) produced if we inject in a volume of 2L at 300 ° C, equimolar quantities of NH3 (g) and HClg) so that the initial total pressure reaches 8.76 atm. The equilibrium constant is K=5.67x10^2.arrow_forwardCalculate the concentration of Cu²+(aq) in a solution that contains 0.020 mol of CuCl, and 0.100 mol of NaCN in 1.0 L. Cu²*(aq) + 4 CN¯(aq) 2Cu(CN);¯(aq) K = 2.0 × 1030 (Hint: Do not overlook the reaction of CN¯ with water to give HCN.)arrow_forward
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