NEET

Solution

What is [H⁺] in mol/L of a solution that is 0.20 M in CH₃COONa and 0.10 M in CH₃COOH? Ka for CH₃COOH = 1.8 × 10^-5.

3.5 ×10^-4
1.1 × 10^-5
1.8 × 10^-5
9.0 × 10^-6

Solution

If pH of a saturated solution of Ba(OH)₂ is 12, the value of its K_sp is :

4.00 × 10^-6 M³
4.00 × 10^-7 M³
5.00 ×10^-6 M³
5.00 × 10^-7 M³

Solution

The dissociation constants for acetic acid and HCN at 25°Care 1.5 × 10^-5 and 4.5 × 10^-10 respectively. The equilibrium constant for the equilibrium CN^– + CH₃COOH ⇌ HCN + CH₃COO^– would be:

3.0 × 10^-5
3.0 × 10^-4
3.0 × 10⁴
3.0 × 10⁵

Solution

Solution

Solution

Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture ?

1.11× 10^-4 M
3.7 × 10^-4 M
3.7 × 10^–3 M
1.11× 10^–3 M

Solution

Solution

K_sp of Ca(OH)2 is 4.0 × 10^–6. At what minimum pH, Ca²⁺ ions start precipitating in 0.01 M CaCl₂?

12 – log 2
12 + log 2
2– log 2
2 + log 2

Solution

K_sp[Ca(OH)₂] = 4.0 ×10^–6 =[Ca²⁺] [OH^–]² = 0.01 ×[OH^–]² ⇒[OH^–] = 2×10^–2 ;
pOH = – log 2 × 10^–2= 2–log 2; pH =14–(2–log2)= 12 + 2 log 2

At certain temperature Kw for water 4.0 × 10^–14. Which of the following is wrong for pure water at this temperature?

pH = 6.699 ;water is acidic
pH = 6.699 ; water is neutral
pOH =6.699 ; water is neutral
pH + pOH = 13.398 ; water is neutral

Solution

[H⁺] = [OH^-] = \(\sqrt{40 \times 10^{-14}}\) = 2.0 × 10^-7
pH = pOH = -log 2 × 10^-7 = 6.699

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