Molarity of a solution of `NH_(4)OH` which is `34%` by weight and whose density is `0.6 (gm)/(ml)` is:
`2.04 M`
`4.08 M`
`5.82 M`
`12.0 M`

A 7.0 M solution of KOH in water contains 28% by mass of KOH. What is density of solution in gm/ml ?

The pH of a 0.1M solution of NH_(4)OH (having dissociation constant K_(b) = 1.0 xx 10^(-5)) is equal to

Calculate pH of 0.001 M NH_(4)OH , when it is 1% dissociated in the solution :

Find molality of aqueous solution of CH_(3)COOH whose molarity is 2M and density d = 1.2g//mL "Hint":m=(M)/(d-MM_(s))xx1000 Where d = density in gL^(-1) , ,M = Molartity, m = molality, M_(S) = molar mass of solute .

Find molality of aqueous solution of CH_(3)COOH whose molarity is 1M and density d = 1.2g//mL "Hint":m=(M)/(d-MM_(s))xx1000 Where d = density in gL^(-1) , ,M = Molartity, m = molality, M_(S) = molar mass of solute .

Molarity of Mg(OH)_2 is 18 M. Its density is 1..6 g/ml, hence molality is :

The molarity of a solution obtained by mixing 750 mL of 0.5 (M) HCl with 250 mL of 2(M) HCl will be:

The pH of 0.2 M aqueous solution of NH_4Cl will be (pK_b of NH_4OH = 4.74, log 2 = 0.3)

Assertion :- The molarity of a certain solution is always greater than molority. If density of solution is nearly 1gm//ml . Reason :- m=(1000M)/(1000M-MxxM_(solute))

The density of NH_(4)OH solution is 0.6g//mL . It contains 34% by weight of NH_(4)OH . Calculate the normality of the solution: