The emf of the cell,               Tl(s) | Tl+(aq) (0.0001 M) || Cu2+(aq) (0.01M) | Cu(s) is 0.83 V                The emf of this cell will be increased by :–Increasing the concentration of Cu2+ ionsDecreasing the concentration of Tl+Increasing the concentration of both(A) & (B) both

The emf (electromotive force) of a cell is determined by the Nernst equation, which relates the reduction potential of a half-cell reaction to the standard electrode potential, temperature, and concentrations of the reactants and products.

The Nernst equation is: E = E° - (RT/nF) * ln(Q)

Where: E is the cell potential, E° is the standard cell potential, R is the gas constant, T is the temperature, n is the number of moles of electrons transferred in the reaction, F is the Faraday constant, and Q is the reaction quotient, which is the ratio of the concentrations of the products to the reactants.

In the given cell, the reaction is:

Tl(s) -> Tl+(aq) + e- (oxidation half-reaction) Cu2+(aq) + 2e- -> Cu(s) (reduction half-reaction)

The overall cell reaction is:

Tl(s) + Cu2+(aq) -> Tl+(aq) + Cu(s)

From the Nernst equation, we can see that increasing the concentration of the products (Tl+ in this case) or decreasing the concentration of the reactants (Cu2+ in this case) will decrease the value of Q, which will increase the cell potential (E).

Therefore, the emf of the cell will be increased by both increasing the concentration of Cu2+ ions and decreasing the concentration of Tl+ ions. So, the correct answer is (A) & (B) both.