Question

calculate the hydrogen and hydroxyl Ion concentration in 0.01m HNO3​

Answer 1

Answer:At 25 degree Celsius, we know that, pH + pOH=14

pH and pOH are the negative logarithms of the concentrations of hydrogen(or hydronium) ion and hydoxide ion respectively.

Hence, for the given solution, since NaOH is a strong base and ionises completely, the concentration of hydroxide ions in it is 0.01 M.

Hence, pOH= -log(0.01) = 2

So, pH of the given solution at 25 degree Celsius = 14 - pOH = 14 - 2 = 12

Note that we cannot calculate the pH of NaOH like we do so for acids since NaOH does not produce hydrogen ions in solution.

Also, the pH would change if the temperature is changed, as the ionic product of water changes with temperature.

Explanation:

Answer 2

Answer:

Hydrogen Ion concentration [H⁺] = 1 X 10⁻² M or 0.01 M

Hydroxyl Ion concentration [OH⁻] = 1 X 10⁻¹² M

Explanation:

Given

Molarity of HNO₃ = 0.01 M

Hydrogen Ion concentration [H⁺] = ??

Hydroxyl Ion concentration [OH⁻] = ??

Solution

HNO₃ is a strong acid and it completely dissociates when dissolved in water. Therefore, the concentration of Hydrogen Ion is same as the molarity of HNO₃ solution.

Hydrogen Ion concentration [H⁺] = 0.01 M

[H⁺] = 1 X 10⁻² M

where as for hydroxyl ion concentration [OH⁻]

as we know that,

Kw = [H⁺] [OH⁻]

where at 25 °C Kw = 1 X 10⁻¹⁴

Hydroxyl Ion concentration [OH⁻] = Kw / [H⁺]

[OH⁻] = 1 X 10⁻¹⁴/0.01

[OH⁻] = 1 X 10⁻¹² M

Concentration of  [OH⁻] is very small as compared to [H⁺] ion concentration so can be neglected.