What is $[H^{+}][H^+]$ of a solution that is 0.1 M HCN and 0.2 M NaCN?($K_{a}K\_a$ for $HCN=6.2\times 10^{-10}HCN\; =\; 6.2\; \backslash times10^\{-10\}$)

The pH of a buffer containing equal molar concentrations of a weak base and its chloride ($K_{b}K\_b$ for weak base $=2\times 10^{-5},=\; 2\; \backslash times\; 10^\{-5\}\; ,$ log 2 = 0.3) is

Solution of 0.1 N $N{H}_{4}OHNH\_4OH$ and 0.1 N $N{H}_{4}ClNH\_4Cl$ has pH 9.25. Then $p{K}_{b}pK\_b$ of $N{H}_{4}OHNH\_4OH$ is

The most important buffer in the blood consists of :

The pH of blood is maintained by the balance between $H_{2}C{O}_{3}H\_2CO\_3$ and $NaHC{O}_{3}NaHCO\_3$. If the amount of $C{O}_{2}CO\_2$ in the blood is increased, how will it effect the pH of blood

If equal volumes of $BaC{l}_{2}BaCl\_2$ and NaF solutions are mixed, which of these combinations will not give a precipitate? $K_{sp}K\_\{sp\}$ of $Ba{F}_2=1.7\times 10^{-7}BaF\_2\; =\; 1.7\; \backslash times10^\{-7\}$

The solubility products of $Al(OH{)}_{3}Al(OH)\_3$ and $Zn(OH{)}_{2}Zn(OH)\_2$ are $8.5\times 10^{-23}8.5\; \backslash times\; 10^\{-23\}$and $1.8\times 10^{-14}1.8\; \backslash times\; 10^\{-14\}$, respectively. If $N{H}_{4}OHNH\_4OH$ is added to a solution containing $A{l}^{+3}Al^\{+3\}$ and $Z{n}^{+2}Zn^\{+2\}$ ions, then substance precipitated first is :

$C{a}_3(P{O}_4{)}_{2}Ca\_3(PO\_4)\_2$ is insoluble in water. On adding a few drops of HCl to solid $C{a}_3(P{O}_4{)}_{2}Ca\_3(PO\_4)\_2$ in contact with water, the solid dissolves. What is the reason?

Why does only $A{s}^{3+}As^\{3+\}$get precipitated as $A{s}_2{S}_{3}As\_2S\_3$ and not $Z{n}^{2+}Zn^\{2+\}$as ZnS when $H_{2}SH\_2S$ is passed through an acidic solution containing $A{s}^{3+}As^\{3+\}$ and $Z{n}^{2+}Zn^\{2+\}$?

When HCl (s) is passed through a saturated solution of common salt, pure NaCl is precipitated because :