Calculate [Cu+] and [CN-] in a 0.500 M solution of [Cu(CN)2]-. Kf = 1.0 × 1016

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A: Reaction: Ag+ +2CN- ⇋ [Ag(CN)]- 1 mole of AgNO3 reacts with 2 moles of KCN to form 1 mole of…

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Q: Calculate the free metal concentration (in ppm) of each of the following solutions.a. A solution…

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Q: What is the normality of 0.050 M Cu2+ solution based on the reaction below? Cu2+ (ag)+ 2e- Cu (s)

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Q: 1. Calculate the concentration of Zn²* in a 0.30M solution of [Zn(CN)4]². Kr[Zn(CN)4] ² = 1 x 1019…

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Q: Calculate AG for the dilution of aqueous HCl from 2.17 M to 0.276 M at 25°C.

A: Given that HCl has to be diluted from a concentration of 2.17 M to 0.276 M at 25°C. Therefore, the…

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Q: What [Ag+] is required to reduce [CO32−] to 8.2 × 10–4 M by precipitation of Ag2CO3?

A: As the initial concentration of [CO32-] is not given,we will take,initial concentration of [CO32-] =…

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Q: Complete the balanced dissociation equation for the compound below in aqueous solution. If the…

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Q: The ammonia ion NH4* has a Ką of 5.6 x 1010, What is the Kp for the base ammonia? 0.000017

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Q: Calculate [Cu+] and [CN-] in a 0.500 M solution of [Cu(CN)2]-. Kf = 1.0 × 1016.

A: Given, Kf = 1.0 × 1016.

Q: Balanced net ionic equation for: S2O32- and 0.2 M Ba (NO3)2 NO3- and 0.1 M AgNO3 I- and 0.2 M…

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Q: What is the pH value of the solution containing 0.085 M HNO2 and 0.1 M KNO2? (Ka: 4,5x10-4)

A: Given: Concentration of  HNO2= 0.085M Concentration of KNO2=0.1M Ka=4.5×10-4

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Q: -2. Describe how 500 mL of standard 0.0100 M Na* solution can be prepared from primary standard…

A: Given-> Volume of Na+ = 500 ml Molarity of Na+= 0.0100M Molar mass of Na2CO3 = 105.99 gm/mole

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Q: The solubility product for Cu(OH)₂(s) is 1.6x 10-19. Calculate the value of 8° for the following…

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Q: The equilibrium constant for the reaction Hg2+(aq) + 2Cl−(aq) ⇌ HgCl2(aq) is 1.6 × 1013. Is HgCl2 a…

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Q: 2. Write net ionic equations for the hydrolysis of the given ions with H2O. a. NH3: b. HBr: c. S2-…

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Q: 4. Which of the following statement is true A. The change in potential in the equivalence-point…

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A: Given : Concentration of Ni(CN)42- = 0.71 M And Kf of Ni(CN)42- = 1.7 X 1030  The formation reaction…

Q: Calculate [Cu+] and [CN-] in a 0.700 M solution of [Cu(CN)2]- (Kf = 1.9×1016) [Cu+] = ______ M…

A: Kf = 1.9 × 1016 Concentration of [Cu(CN)2]- = 0.700 M Concentration of Cu2+ = ? Concentration of CN-…

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Q: A 0.0320 M solution of a weak base has a pH of 9.45. Determine the Kp of this weak base.

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Q: Calculate the pH of a 0.859 M NaF solution. Assume Ka(HF) = 1.0 x 10-4

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Q: What is the concentration of Be(OH)2 (aq) in a solution in which the concentrations of Be2+ and OH−…

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Q: The acid ionization constant for Fe(H2O),²*(aq) is 3.0×10-6. Calculate the pH of a 0.0170 M solution…

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