Waht is the pH of a 250.0 mL sample of 0.105 M HNO2?

Question

Question

Answer 1

Answer #1

The ionisation of HNO is She as pea follane - I H₂ot (aq) + No, caq.) & H₂O (W - HNO₂ (ar) Here ha is Ka pae requisite 4.6 x

Answer 2

Similar Homework Help Questions

a) A 41.0 mL sample of 0.194 M HNO2 is titrated with 0.220 M KOH. (Ka...

a) A 41.0 mL sample of 0.194 M HNO2 is titrated with 0.220 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH. b) A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 56.7 mL 0.200 M HNO3.
Consider the titration of a 21.0 −mL sample of 0.105 M HC2H3O2 with 0.130 M NaOH....

Consider the titration of a 21.0 −mL sample of 0.105 M HC2H3O2 with 0.130 M NaOH. Determine each of the following. . a. The initial pH b. The volume of added base required to reach the equivalence point c. The pH at 5 mL of added base d. The pH at one-half the equivalence point e. The pH at the equivalence point
Consider the titration of a 21.0 – mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH

Consider the titration of a 21.0 – mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each of the following. Part A the initial pH Part B the volume of added base required to reach the equivalence pointPart C the pH at 4.00 mL of added basePart D the pH at one-half of the equivalence point Part E the pH at the equivalence point

A 42.0 mL sample of 0.120 M HNO2 is titrated with 0.214 M KOH. (Ka for...

A 42.0 mL sample of 0.120 M HNO2 is titrated with 0.214 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH.
A 41.0 mL sample of 0.174 M HNO2 is titrated with 0.264 M KOH. (Ka for...

A 41.0 mL sample of 0.174 M HNO2 is titrated with 0.264 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH.
| 22) - 22) Consider the titration of a 20.0-ml sample of 0.105 M HC2H302 with...

| 22) - 22) Consider the titration of a 20.0-ml sample of 0.105 M HC2H302 with 0.125 M NaOH. Determine the pH at the equivalence point. A) 2.86 B) 4.74 C) 8.75 D) 12.17

125 mL of 0.010 M HI. 16.45 Calculate [OH] and pH for (a) 1.5 x 103MSr(OH) 2, ב- (b) 2.250 g of LIOH in 250.0 mL of...

125 mL of 0.010 M HI. 16.45 Calculate [OH] and pH for (a) 1.5 x 103MSr(OH) 2, ב- (b) 2.250 g of LIOH in 250.0 mL of solution, (c) 1.00 mL of 0.175 M NAOH diluted to 2.00 L, (d) a solution formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of 9.5 x 102 M Ca (OH)2.
What is the pH of 65 mL of 0.0685 M HNO2?

What is the pH of 65 mL of 0.0685 M HNO2?
A 109.2 mL sample of 0.105 M methylamine (CH3NH2;Kb=3.7×10−4) is titrated with 0.250 M HNO3. Calculate...

A 109.2 mL sample of 0.105 M methylamine (CH3NH2;Kb=3.7×10−4) is titrated with 0.250 M HNO3. Calculate the pH after the addition of each of the following volumes of acid. a.0.0 mL Express the pH to two decimal places. b. 22.9 mL c.45.9ml d.68.8ml

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with...

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3. The Kb for NH3 is 1.8 × 10-5. 8.25 9.18 10.83 9.50