
Consider:
\[ \left( \sqrt{3} + \sqrt{2} \right)^x + \left( \sqrt{3} - \sqrt{2} \right)^x = 10 \]
Let:
\[ \left( \sqrt{3} + \sqrt{2} \right)^x = t \]
Thus:
\[ \left( \sqrt{3} - \sqrt{2} \right)^x = \frac{1}{t} \]
Substitute and simplify:
\[ t + \frac{1}{t} = 10 \]
Multiplying through by \( t \) gives:
\[ t^2 - 10t + 1 = 0 \]
Solving this quadratic equation:
\[ t = \frac{10 \pm \sqrt{100 - 4}}{2} = \frac{10 \pm \sqrt{96}}{2} = \frac{10 \pm 4\sqrt{6}}{2} = 5 \pm 2\sqrt{6} \]
Since:
\[ \left( \sqrt{3} + \sqrt{2} \right)^x > 0, \quad t = 5 + 2\sqrt{6} \]
Thus, the corresponding values of \( x \) are:
\[ x = 2 \quad \text{or} \quad x = -2 \]
Number of solutions = 2.
The molar conductance of an infinitely dilute solution of ammonium chloride was found to be 185 S cm$^{-1}$ mol$^{-1}$ and the ionic conductance of hydroxyl and chloride ions are 170 and 70 S cm$^{-1}$ mol$^{-1}$, respectively. If molar conductance of 0.02 M solution of ammonium hydroxide is 85.5 S cm$^{-1}$ mol$^{-1}$, its degree of dissociation is given by x $\times$ 10$^{-1}$. The value of x is ______. (Nearest integer)
x mg of Mg(OH)$_2$ (molar mass = 58) is required to be dissolved in 1.0 L of water to produce a pH of 10.0 at 298 K. The value of x is ____ mg. (Nearest integer) (Given: Mg(OH)$_2$ is assumed to dissociate completely in H$_2$O)
Sea water, which can be considered as a 6 molar (6 M) solution of NaCl, has a density of 2 g mL$^{-1}$. The concentration of dissolved oxygen (O$_2$) in sea water is 5.8 ppm. Then the concentration of dissolved oxygen (O$_2$) in sea water, in x $\times$ 10$^{-4}$ m. x = _______. (Nearest integer)
Given: Molar mass of NaCl is 58.5 g mol$^{-1}$Molar mass of O$_2$ is 32 g mol$^{-1}$.