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12 Dec 2019

Suppose you have a sample of 25.0 mL of 0.01M HCl solution. HCl is a strong acid and it completely dissociates in water. Calculate the pH of this solution (pH= -log[H3O+]).

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Trinidad Tremblay
Trinidad TremblayLv2
13 Dec 2019

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Related questions

A sample of nitric acid is prepred which contains 0.0030 moles of HNO3 in water to make 1500 mL of solution. This is a strong acid and completely dissociates:

HNO3 + H2O รขย†ย’ H3O+ + NO3-

Caluculate the molarity of the solution (moles/liter), its [H3O+], and its pH value.

1. Calculate the anticipated pH for each of the solutions thatresulted when you added HCl or NaOH to the "water" beaker (a beakercontaining 50 mL of DI water and chemical indicators).

2. Calculate the concentration of H3O+ ion for each of thesolutions. Enter the data in the tables.


Here is the first row of each table, after I see how it's done,I can do the rest.


Volume of HCl added | Anticipated pH | Experimentally determinedpH | Experimentally determined [H3O+]

5ml | ??? | 2.24 | ??? |



Volume of NaOH added | Anticipated pH | Experimentallydetermined pH | Experimentally determined [H3O+]

5ml | ??? | 11.45 | ??? |


Given:

Kw is [H3O+][OH-] = 1.0 x 10^-14

pH = -log[H3O+]

HCl concentration and NaOH concentration: 0.01M


Please show steps, any help is appreciated! :)

Please help!**** for each of the indicated concentration strong or weak acids determine concentrations of acid [HA], hydronium ion H3O and pH of the solution (ka,Kb values on table)

15mL of 0.500 M HCL mixed with water to make 2.00 L of solution

and

10mL of 0.50 M acetic acid mixed with water to make 25.0 ml solution .

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