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))`

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) )

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) .

The pH of a solution obtained by mixing 100mL of 0.1M HCI and 9.9mL of 0.1M 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 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

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) .