`10xx0+10+10-10`

At what pH will a 1.0 xx 10^(-3)M solution of an indicator with K_(b) = 1.0 xx 10^(-10) changes colour?

The pH of a solution of NH_4Cl is 4.86 .Calculate the molar concentration fo the solution if K_b= 1.0 xx 10^(-5) and K_w = 1.0 xx 10 ^(-14)

Multiply : 10. 1001 xx 10. 01

What is the percentage hydrolysis of CH_3COONa in 0.01 M Solution ? (K_a= 1.78 xx 10 ^(-5) and K_w = 1.0 xx 10 ^(-14))

What would be the solubility of silver chloride in 0.10M NaCI solution? K_(sp) for AgCI = 1.20 xx 10^(-10)

The first and second dissociation constant of an acid H_2A are 1.0 xx 10 ^(-5) and 5.0 xx 10^(-10) respectively . The overall dissociation constant of the acid will be : 5.0 xx 10^(-5) 5.0 xx 10 ^(-15) 5.0 xx 10 ^(-15) 0.2 xx 10 ^(5)

In a carbon monoxide molecule, the carbon and the oxygen atoms are separted by a distance 1.12 xx 10^(-10) m. The distance of the centre of mass from the carbon atom is A. 0.64 xx 10^(-10)m B. 0.56xx10^(-6) m C. 0.51 xx 10^(-10) m D. 0.48 xx 10^(-10) m

An aqueous solution contains 0.10 MH_2 S and 0.20 M HCl if the equilibrium constants for the formation of HS^(-) " from " H_2S " is " 1.0 xx 10^(-7) and " that of " S^(2-) " from " HS^(-) ions is 1.2 xx 10 ^(-13) then the concentration of S^(2-) ions in aqueous solution is 5 xx 10 ^(-8) 3 xx 10 ^(-20) 6 xx 10 ^(-21) 5 xx 10 ^(-19)

Calculate the percentage hydrolysis of decinormal solution of ammonium acetate given that k_(a) = 1.75 xx 10^(-5), K_(b) =1.80 xx 10^(-5) and K_(w) = 1.0 xx 10^(-14)

Calculate the percentage hydrolysis of decinormal solution of ammonium acetate given that k_(a) = 1.75 xx 10^(-5), K_(b) =1.80 xx 10^(-5) and K_(w) = 1.0 xx 10^(-14)