A solution containing `2.7 xx 10^-3` mol of `A^(2+)` irons required `1.6 xx 10^(-3)` mole of `MnO_4^-` for the oxidation of `A^(2+)` to `AO_3^-` the medium used is :

A solution contaning 2.7 xx 10^(-3) mol of A^(2+) "ion required" 1.6 xx 10^(-3)mol of MnO_(4)^(2-) for the oxidation of A^(2+) "to" AO_(3)^(-) the medium is:

2.68xx10^(-3) moles of solution containing anion A^(n+) require 1.61xx10^(-3) moles of MnO_(4)^(-) for oxidation of A^(n+) to AO_(3)^(-) in acidic medium. What is the value of n ?

2.68xx10^(-3) moles of solution containing anion A^(n+) require 1.61xx10^(-3) moles of MnO_(4)^(-) for oxidation of A^(n+) to AO_(3)^(-) in acidic medium. What is the value of n ?

4 " mol of "a solution A^(n+) requires 1.6 " mol of " MnO_4^(-) ions for the oxidation of A^(n+) to AO_3^(ɵ) in acidic medium the value of n is (a). 1 (b). 2. (c). 3. (d). 4.

1.0L of solution which was in equilibrium with solid mixture of AgC1 and AgC1 and Ag_(2)CrO_(4) was found to contain 1xx 10^(-4) mol of Ag^(o+) ions, 1.0 xx 10^(-6) mol of C1^(Θ) ions and 8.0 xx 10^(-4) moles of CrO_(4)^(2-) ions. Ag^(o+) ions added slowely to the above mixture (keeping volume constant) till 8.0 xx 10^(-7) mol of AgC1 got precipitated. How many moles of Ag_(2)CrO_(4) were also precipitated?

For 1.34xx10^(-3) moles of KBrO_3 to reduce into bromide 4.02 xx 10^(-3) mole of X^(n+) ion is needed. New oxidation state of X is:

An element A in a compound ABD has oxidation number A^(n-) . It is oxidised by Cr_(2)O_(7)^(2-) in acid medium. In the experiment 1.68xx10^(-3) moles of K_(2)Cr_(2)O_(7) were used for 3.26xx10^(-3) moles of ABD . The new oxidation number of A after oxidation is:

Rate constant k = 1.2 xx 10^(3) mol^(-1) L s^(-1) and E_(a) = 2.0 xx 10^(2) kJ mol^(-1) . When T rarr oo :

6 xx 10^(-3) mole K_2 Cr_2 O_7 reacts completely with 9 xx 10^(-3) mole X^(n+) to given XO_3^- and Cr_^(3+) . The value of n is :

A solution contains 2.3 xx 10^(-3) M Ag NO_(3) . What concentration of NaCl will be required to initiate the precipitation of AgCl. The solubility product of AgCl is 2.8 xx 10^(-10) ?