Advertisements
Advertisements
Question
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Advertisements
Solution
For 0.3 g of NaOH dissolved in water to give 200 mL of solution:
\[\ce{NaOH -> Na^+_{(aq)} + OH^-_{(aq)}}\]
`["NaOH"] = 0.3 xx 1000/200 = 1.5 "M"`
`["OH"_("aq")^-] = 1.5 "M"`
Then `["H"^+] = 10^(-14)/1.5`
`= 6.66 xx 10^(-13)`
`"pH" = - log(6.66 xx 10^(-13))`
= 12.18
APPEARS IN
RELATED QUESTIONS
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the pKa of bromoacetic acid.
The solubility of Sr(OH)2 at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution.
Calculate the pH of the resultant mixtures: 10 mL of 0.01M H2SO4 + 10 mL of 0.01M Ca(OH)2.
Choose the most correct answer :
Blood in the human body is highly buffered at a pH of ________.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
What is the pOH if the hydrogen ion concentration in solution is 1 × 10–3 mol dm–3?
When CuSO4 solution in water is treated with concentrated HCl it turns _______.
Aqueous solution of ____________ will turn red litmus blue.
The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively.
Neutral solutions have the pH of ______.
A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of \[\ce{NH^+_4}\] is 0.20 M. If the equilibrium constant, Kb tor NH3 equals 1.8 × 10-5, what is the pH of the solution?
Define pOH.
Define pH.
Define pOH.
Derive a relationship between pH and pOH.
Define pH.
Define pOH.
Derive relationship between pH and pOH.
