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Calculate the solubility of AgCN in a bu...

Calculate the solubility of `AgCN` in a buffer solution of `pH 3.0`. Assume that no cyano complex is formed `K_(sp) AgCN = 2.2 xx 10^(-16), K_(a) HCN = 6.2 xx 10^(-10)`.

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AI Generated Solution

To calculate the solubility of `AgCN` in a buffer solution of `pH 3.0`, we will follow these steps: ### Step 1: Write the Dissociation Reactions AgCN dissociates in water as follows: \[ \text{AgCN (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{CN}^- (aq) \] HCN dissociates in water as follows: \[ \text{HCN (aq)} \rightleftharpoons \text{H}^+ (aq) + \text{CN}^- (aq) \] ...
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Calculate the solubility of AgCN in a buffer solution of pH 3.00 assuming no complex formation, K_(a) (HCN)=6.2 xx 10^(-10) and K_(sp) (AgCN)=2.2 xx 10^(-16) .

Calculate the solubility of AgCN in a buffer solution of pH 3*00 . K_(sp) for AgCN is 2.2xx10^(-16) and K_(a) for HCN is 6.2xx10^(-12) .

Knowledge Check

  • The solubilty of AgCN in a buffer solution of pH = 3 is x . The value of x is [Assume : No cyano complex is formed, K_(sp)(AgCN)=2.2xx10^(-16) and K_a(HCN)=6.2xx10^(-10)]

    A
    `0.625xx10^(-6)`
    B
    `1.9xx10^(-5)`
    C
    `2.2xx10^(-16)`
    D
    `1.6xx10^(-6)`

  • What is the solubility of Al(OH)_(3) , ( K_(sp)=10^(-33) ) in a buffer solution of pH=4?

    A
    `10^(-3)`M
    B
    `10^(-6)`M
    C
    `10^(-4)`M
    D
    `10^(-10)`M

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    Calculate the solubility of AgCN in a buffer solution of pH = 3 , Given K_(sp) of AgCN = 1.2 xx 10^(-16) and K_(a) for HCN = 4.8 xx 10^(-10) .

    Calculate the solubility of CaF_(2) in a solution buffered at pH = 3.0. K_(a) for HF = 6.3 xx 10^(-4) and K_(sp) of CaF_(2) = 3.45 xx 10^(-11) .

    Equal volumes of 0.02 M AgNO_3 and 0.02 M HCN were mixed. Calculate [Ag^+] at equilibrium assuming no cyano-complex formation. K_(sp) (AgCN)=2.2 xx 10^(-16), K_(a) (HCN)=6.2 xx 10^(-10) .

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