One half cell in a voltaic cell is constructed by dipping silver rod in $$\text{AgNO}_3$$ solution of unknown concentration, other half cell is Zn rod dipped in 1 molar solution of $$\text{ZnSO}_4$$. A voltage of $$1.60\,\text{V}$$ is measured at $$298\,\text{K}$$ for this cell. What is the concentration of $$\text{Ag}^+$$ ions used in terms of $$\log x$$ $$(x = [\text{Ag}^+])$$?

$$E^\ominus_{\text{Zn}^{2+}/\text{Zn}} = -0.76\,\text{V}, \quad$$ $$E^\ominus_{\text{Ag}^{+}/\text{Ag}} = +0.80\,\text{V}, \quad$$ $$\frac{2.303RT}{F} = 0.059\,\text{V}$$