Advertisements
Advertisements
प्रश्न
Calculate the pH of the following solution:
0.3 g of NaOH dissolved in water to give 200 mL of solution.
Advertisements
उत्तर
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
संबंधित प्रश्न
Assuming complete dissociation, calculate the pH of the following solution:
0.002 M KOH
The pH of 10−8 M of HCl is ______.
Answer the following in one sentence:
The pH of a solution is 6.06. Calculate its H+ ion concentration.
Answer the following :
The pH of rainwater collected in a certain region of Maharashtra on a particular day was 5.1. Calculate the H+ ion concentration of the rainwater and its percent dissociation.
Which of the following when dissolved in water results in neutral solution?
The pH of 0.001 M HCl solution is ______.
The least basic hydroxide from the following is:
Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations.
i. 60 mL `"M"/10` HCl + 40 mL `"M"/10` NaOH
ii. 55 mL `"M"/10` HCl + 45 mL `"M"/10` NaOH
iii. 75 mL `"M"/5` HCl + 25 mL `"M"/5` NaOH
iv. 100 mL `"M"/10` HCl + 100 mL `"M"/10` NaOH
pH of which one of them will be equal to 1?
Equal volumes of three acid solutions of pH 1, 2 and 3 are mixed in a vessel. What will be the H+ ion concentration in the mixture?
The pH of 10−5 M KOH solution will be ____________.
Neutral solutions have the pH of ______.
If pH of a solution is 3.12, what would be the concentration of H+ ion?
The mole fraction of the solute molal aqueous solution is:
Derive the relationship between pH and pOH.
Derive a relationship between pH and pOH.
Define pH.
Define pOH.
