« previous 3 of 3 return to assignment Part A Ch15 16: Chemical Equilibrium. Seg

Question

« previous 3 of 3 return to assignment Part A Ch15 16: Chemical Equilibrium. Seg3: Equilibria Affected by pH Changes 114-OL-Course What is the pH of a neutral solution? 7 Submit The pH of a solution is the negative log of the hydronium ion concentration: My Answers Give Up Correct In pure water, or in any neutral solution, the hydronium concentration is 1.0 x 10 M due to the autoionization of water: Part B In an acidic solution the hydronium concentration is 107 M, and the pH is than 2H20(1)-. H3O+ (aq) + OH (aq) Keq = 10-14 -than 7.0 Please Choose greater, greater greater, less less, less less, greater Gastric juice wers Give Up Cola, vinegar LLO 1X10- 1x10-4 4.0 10.0 10-30 ain Baking soda Milk of magnesia Household ammonia NaOH, 01M Part C In a basic solution the hydroxide concentration is 10- M, and the pH is than than 7.0 1 10- 11.0 3.o -1x10-.. 120) 20 ·x10" K10-1 1x10-1 | Please Choose Submit My Answers Give Up Determine the pH of the following solutions Part D -Calculate the pH of a solution with a hydronium concentration of 103M Submit My Answers Give Up Part E Calculate the pH of a solution with a hydronium concentration of 10-12M. Submit My Answers Give Up Part F Calculate the pH of a 0.010 M HCI solution. Hints Submit My Answers Give Up

Explanation / Answer

part A :7

All neutral solutions have a pH of 7. This is the solution where [H+] and [OH-] are same.

Part B: greater, less

In acidic solution, [H+] or [H3O]+ is high. As pH= -log[H+], pH value is less, and in basic solutions [OH-] is more compared to [H+], thus pH is high.

Part C: greater, greater

Pard D: 3

pH = -log [H+]

= -log [10 -3]

=3

Part E: 12 (similar explanation as above)

Part F: 2 (similar explanation as D)

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