The concentration of hydroxyl ion in a solution left after mixing 100 mL of 0.1 M `MgCl_(2)` and 100 mL of 0.2 M NaOH:
(`K_(sp)` of `Mg(OH)_(2)=1.2xx10^(-11)`)

The concentration of hydroxyl ion in a solution left after mixing 100 mL of 0.1M MgCl_(2) and 100 mL of 0.2M NaOH is: (K_(SP)of Mg(OH)_(2)=1.2xx10^(-11))

Calculate the concentration of hydroxyl ion in a solution left after mixing 100 ml of 0.1 M Mgcl_2 and 100 ml of 0.2 M NaOH [ K_sp of Mg(OH_2) = 1.2xx 10^(-11 )]

Calculate the [OH^(-)] of a solution after 100 mL of 0.1 M MgCl_(2) is added to 100 mL 0.2 M NaOH K_(sp) of Mg(OH)_(2) is 1.2 xx10^(-11) .

a. Will a precipitate of Mg(OH)_(2) be formed in a 0.001M solution of Mg(NO_(3))_(2) if the pH of solution is adjusted to 9.K_(sp) of Mg(OH)_(2) = 8.9 xx 10^(-12) . b. Calculate pH at which Mg(OH)_(2) begin to precipitae form a solution containing 0.1M Mg^(2+) ions. K_(sp) of Mg(OH)_(2) =1 xx 10^(-11) . c. Calculate [overset(Theta)OH] of a solution after 100mL of 0.1M MgC1_(2) is added to 100mL of 0.2M NaOH. K_(sp) Mg(OH)_(2) = 1.2 xx 10^(-11) .

The normality of solution obtained by mixing 100 ml of 0.2 M H_(2) SO_(4) with 100 ml of 0.2 M NaOH is

The normality of solution obtained by mixing 100 ml of 0.2 M H_(2) SO_(4) with 100 ml of 0.2 M NaOH is

The normality of solution obtained by mixing 100 ml of 0.2 M H_(2) SO_(4) with 100 ml of 0.2 M NaOH is

The hydrogen ion concentration and pH of the solution made by mixing 100 mL of 1.0 M HNO_(3) with 100 mL of 0.8 M KOH, are