(a)
Interpretation:
The solubility product of saturated solution of copper carbonate is to be stated.
Concept introduction:
In a
(b)
Interpretation:
The solubility product of saturated solution of zinc carbonate is to be stated.
Concept introduction:
In a chemical reaction, when the rates of both forward and reverse reaction are equal then the chemical reaction is said to be at equilibrium. They are reversible in nature. Equilibrium constant is denoted as
(c)
Interpretation:
The solubility product of saturated solution of aluminium carbonate is to be stated.
Concept introduction:
In a chemical reaction, when the rates of both forward and reverse reaction are equal then the chemical reaction is said to be at equilibrium. They are reversible in nature. Equilibrium constant is denoted as
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Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- The reaction for the formation of diammine silver ion is as follows: Ag + (aq) + 2 NH3 (aq) <--->Ag(NH3)2 + Write the equilibrium constant expression for the reaction:arrow_forwardConsider 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?arrow_forwardIn a solution of 0.73 M Ag(NH3)2, how much free NH3 is in solution at equilibrium? Ag+(aq) + 2NH3(aq) ⇌ Ag(NH3)2+(aq) Kf = 1.7 x107arrow_forward
- 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.arrow_forwardpH and Solubility Is the solubility of the following compounds increased in an acidic solution? (a) Ca(OH)2 (b) Mg3(PO4)2 (c) PbBr2arrow_forwardWhat is the equilibrium expression for the following reaction? Zn(s) + 2NAOH(aq) + 2H2O(e) = NazZn(OH)4(aq) + H2(g)arrow_forward
- The ionic compound magnesium hydroxide, which is found in the over-the-counter consumer product Milk of Magnesia™,has the formula Mg(OH)2. Magnesium hydroxide dissolves in water according to the following equation:Mg(OH)2(s) ←→ Mg2+(aq) + 2OH–(aq)Write the solubility product expression for magnesium hydroxidearrow_forwardCalculate the equilibrium concentration of Ag+(aq) in a solution that is initially 0.100 M AgNO3 and 0.800 M NH3 after this reaction takes place: Ag+(aq) + 2NH3(aq) <-------> Ag(NH3)2+(aq) Kf = 1.7 x 107arrow_forwardHydrochloric acid does not appear in either equilibrium reaction, yet it influences the reactions. Explain how it affects the equilibrium of ammonia and phenolphthalein in water and brings about the observed color change. Be specific, and include any relevant chemical equations. Attach a file if necessary. NH3(aq) + H2O (l) ⇄ NH4+(aq) + OH (aq) HCl causes a colorless solutionarrow_forward
- In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC14². Co²+ (aq) is pink and CoC14² (aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: Co²+ (aq) + 4Cl¯¯(aq) ⇒ CoCl² (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of Co²+: O increases. O decreases. O remains the same. O More information is needed to answer this question.arrow_forwardConsider the Gibbs energies at 25 °C. Substance AG; (kJ · mol-!) Ag*(aq) 77.1 Cl^(aq) -131.2 AgCl(s) -109.8 Br¯(aq) -104.0 AgBr(s) -96.9arrow_forwardWrite the equilibrium expression for the reaction Zn2+(aq) + 2 NH3(aq) <--> Zn(NH3)2+(aq)arrow_forward
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