What is `pH` of `Mg(OH)_(2)` solution at `25^(@)C` ? [Given: `K_(sp)[Mg(OH)_(2)]=5times10^(-16)`]

The pH of 0.25 M Ba(OH)_2 solution is:

What will be the pH of 5xx10^(-6)MBa(OH_(2)) solution of 25^(@)C ?

Consider a sturated solution of silver chloride that is in contact with solid silver chloride. The solubility equilibrium can be represented as AgCl(s)hArrAg^(+)(aq.)+Cl^(-)(aq.)," "K_(sp)=[Ag^(+)(aq.)][Cl^(-)(aq.)] Where K_(sp) is clled the solubility product constant or simply the solubility product. In general, the solubility product of a compound is the product of the molar concentrations of the constituent ions, each raised to the power of its stoichiometric coefficient in the equilibrium equation. For concentrations of ions that do not necessarliy correpond to equilibrium conditions we use the reaction quotient (Q) which is clled the ion or ionic prodect (Q) to predict whether a precipitate will from. Note that (Q) has the same for as K_(sp) are QltK_(sp) Unsaturated solution Q=K_(sp) Saturated solution Qgt_(sp) Supersaturated solution, precipitate will from At 25^(@)C, will a precipitate of Mg (OH)_(2) from when a 0.0001 M solution of Mg(NO_(3))_(2) is adjusted to a pH of 9.0 ? At what minimum value of pH will precipition start ? ["Given" : K_(sp)(Mg(OH)_(2))=10^(-11)M^(3)]

The maximum pH of a solution which is having 0.10M in Mg^(2+) and from which Mg(OH)_(2) is not precipated is: (Given K_(sp)Mg(OH)_(2)=4xx10^(-11)M^(3)){log2=0.30}

The pH of Ca(OH)_(2) is 10.6 at 25^(@)C. K_(sp) of Ca(OH)_(2) is

1.75g of solid NaOH is added to 0.25dm^(3) of 0.1M NiCl_(2) solution. Calculate: a. Mass of Ni(OH)_(2) forms b. pH if final solution Given K_(sp) of Ni(OH)_(2) = 1.6 xx 10^(-14)

Will a precipitate of Mg(OH)_(2) be formed in a 0.001 M solution of Mg(NO_(3)) , if the pH of solution is adjusted to 9 ? K_(sp) of Mg(OH)_(2)= 8.9 xx 10^(-12) .

Which of the following concentration of NH_(4)^(+) will be sufficient to present the precipitation of Mg(OH)_(2) form a solution which is 0.01 M MgCl_(2) and 0.1 M NH_(3)(aq) . Given that K_(sp)Mg(OH)_(2)=2.5xx10^(-11) and K_(b) for NH_(3) = 2xx10^(-5) .

Calculate the hydrolysis constant. Degree of hydrolysis and pH of a 0.1 M NH_4Cl solution at 25 ^(@) C Given : K_b " for " NH_4OH= 1.8 xx 10^(-5)

What is the pH of a 0.10 M C_(6)H_(5)O^(-) solution? The K_(a) of C_(6)H_(5)OH is 1.0xx10^(-10)