The `25mL` of a `0.15 `M solution of lead nitrate, `Pb(NO_3)_2` reacts with all of the aluminium sulphate, `Al_2`(SO_4)_3`, present in `20 mL` of a solution. What is the molar concentration of the `AI_2(SO_4)_3` ? `3Pb(NO_3)_2(aq)+AI_2(SO_4)_3(aq)rarr3PbSO_4(s)+2AI(NO_3)_3(aq)`

The 25 mL of a 0.15 M solution of lead nitrate, Pb(NO_(3))_(2) react with all of the aluminium sulphate , Al_(2)(SO_(4))_(3) , present in 200 mL of a solution . What is the molar concentration of the Al_(2)(SO_(4))_(3) , present in 20 mL of a solution . What is the molar concentration of the Al_(2)(SO_(4))_(3) ?

25mL of 0.15M Pb (NO_(3))_(2) reacts completely with 20 mL of Al_(2)(SO_(3))_(2) . The molar concentration of Al_(2)(SO_(4))_(3) will be: 3Pb(NO_(3))_(2)(aq.)+Al_(2)(SO_(4))_(3)(aq.)to3PbSO_(3)(s)+2Al(NO_(3))_(3)(aq.)

On heating Pb(NO_3)_2 the products formed ate :

Pb(NO_(3))_(2)+H_(2)SO_(4) to PbSO_(4)darr+2HNO_(3)

20 ml of 0.2M Al_2(SO_4)_3 is mixed with 20 ml of 6.6 M BaCl_2 the concentration of Cl^- ion in solution is

The number of AI^(3+) ions in 100 mL of 0.15 M solution of AI_2(SO_4)_3 are:

On adding ammonium hydroxide solution to A1_2(SO_4)_3(aq)

What is the equilibrium constant expression for the following reaction ? AI(s) +3H^(+) (aq) hArr AI^(3+) (aq) +3//2 H_(2)(g)

How many gram of Al_(2)(SO_(4))_(3) are present in 100mL of 0.15 m solution of Al_(2)(SO_(4))_(3) ? The density of solution is 1.4g//mL .