3. The salt Ba(CIO), is dissolved in water. a. Is the resulting solution acidic,

Question

3. The salt Ba(CIO), is dissolved in water. a. Is the resulting solution acidic, basic, or neutral? b. Does either ion, Ba* or ClO, , hydrolyze in water? Why or why not? 4. The salt N,H,Cl is dissolved in water. a. Is the resulting solution acidic, basic, or neutral? b. Does either ion, N,H,' or Ch, hydrolyze in water? Why or why not For each ion that hydrolyzes, write the hydrolysis equation. c. Three different indicators are available for the titrations in a?For each indicator, predict the pH of the end point. For each titration in a-c, predict the chemical formola of the salt, relative 5 PH (acidic, basic, or neutral) at the equivalence point, and an appropriate indicator of available Available Indicators I. Thymol blue K 2x 10 II. Bromothymol blue KJ 2x 10 III. Congo red K-1x 10* Titrations End Point pH (yellow blue) (yellow+blue (violet-red) End Point pH End Point pH a. NaOH+ HC,H,O Salt Eq. Point pH- Indicator b. NH,+ HC Salt Eq. Point pH c. NaOH + HCI Salt - Eq. Point pH- Indicator

Explanation / Answer

3.

Ba(ClO4)2 is a salt of strong acid and strong base.

(a) Hence the resulting solution is in neutral nature whose pH = 7.0

(b) SInce the solution is neutral both anion and cation cannot undergo hydrolysis.

No hydrolysis reaction takes palce.

4.

N2H5Cl is a salt of weak base and strong acid.

(a) Since acid is strong but base is weak, the resulting solution is in acidic nature whose pH < 7.0

(b) Since the solution is in acidic nature, cation undergoes hydrolysis.

(c) Cation hydrolysis reaction:

N2H5+ (aq.) + H2O (l) ---> N2H5OH (aq.) + H+ (aq.)

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