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NH(4)CN is a salt of weak acid HCN (K(a)...

`NH_(4)CN` is a salt of weak acid HCN `(K_(a)=6.2xx10^(10))` and a weak base `NH_(4)OH(K_(b)=1.8xx10^(-5))`. A one molar solution of `NH_(4)CN` will be

A

neutral

B

strongly acidic

C

strongly basic

D

weakly basic

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NH_(4)CN is a salt of weak acid HCN(K_(a)=6.2xx10^(-10)) and a weak base NH_(4)OH(K_(b)=1.8xx10^(-5)) . 1 molar solution of NH_(4)CN will be :-

For 10^(-4) M BOH (weak base) , K_(b)=5xx10^(-5)) :

For NH_(3) , K_(b)=1.8xx10^(-5) . K_(a) for NH_(4)^(+) would be

A mixture of weak acid is 0.1M in HCOOH (K_(a) = 1.8 xx 10^(-4)) and 0.1M in HOCN (K_(a) = 3.1 xx 10^(-4)) . Hence, [H_(3)O^(o+)] is

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pH of solution obtained by mixing equal volumes of 0.1M Triethyl amine (K_(b)=6.4xx10^(-5)) & (4)/(45)M NH_(4)OH (K_(b)=1.8xx10^(-5)) will be :

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

Glycine [NH_(2)CH_(2)COOH) is basic and acidic due to presence of -NH_(2) and -COOH group. It acquires a H^(o+) to form overset(o+)NH_(3)COOH , which is a diprotic acid with K_(1) = 4.5 5 xx10^(-3) and K_(2) = 1.7 xx 10^(-10) . In a 0.01M solution of neutral glycine, a. What is the pH and b. What percent of the glycine is in the cationic form at equilibrium?

Total number of solutions from the following which has pHlt7 at 25^(@)C . (K_(a)(CH_(3)COOH)=1.8xx10^(-5),K_(b)(NH_(4)OH)=1.8xx10^(-5)) (i) 10^(-8) MHCl (ii) 0.01 M solution of NH_(4)Cl (iii) 0.01 M solution of CH_(3)COONa (iv) 0.01M solution is B(OH)_(3) (v) 0.01M solution of CH_(3)COONH_(4)

What is pH of 0.02 M solution of ammonium chloride at 25^(@) C ? K_(b) (NH_(3)) = 1.8 xx 10^(-5) .

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