For the given data, the reaction dynamics favour precipitation - True or False? The solution concentration of $B a^{2 +}$ ions is $1 \times 10^{- 3} M$ and that of $S O_{4}^{2 -}$ ions is $2 \times 10^{- 4} M$ ; $K_{s p} (B a S O_{4} )$ $1 \times 10^{- 10}$ .

Q. If you dilute

25.0

mL of

1.5

H C l

500

mL, then the molar concentration of each ions becomes

Y \times 10^{- 3} M

. Here

Y

is:

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If 20mL of an acidic solution of pH 3 is diluted to 100mL, the H+ ion concentration will be.

The correct option is B 2×10−4MpH=3(given)∴[H+]=1×10−3M=1×10−3NN1V1=N2V21×10−3×20=N2×100N2=2×10−4∴[H+]=2×10−4M

If $20$ mL of an acidic solution of pH $3$ is diluted to $100$ mL, the $H^{+}$ ion concentration will be.

The correct option is B $2 \times 10^{- 4} M$
$p H = 3$ (given)
$∴ [H^{+}] = 1 \times 10^{- 3} M = 1 \times 10^{- 3} N$
$N_{1} V_{1} = N_{2} V_{2}$
$1 \times 10^{- 3} \times 20 = N_{2} \times 100$
$N_{2} = 2 \times 10^{- 4}$
$∴ [H^{+}] = 2 \times 10^{- 4}$ M