8. Products are favored in each of the following reactions.HNO3(aq) + CN (aq) HCN(aq) + NO3 (aq)HCN(aq) + OH (aq) H20() + CN (aq)H20() + CH30 (aq):=CH3OH(aq) + OH (aq)Identify the weakest acid and explain your answer.Identify the strongest base and explain your answer.9. The salt of a weak acid HA has the formula NaA. The pH of 0.135 MNaA is 10.7. Calculate the Ka for HA. 5. Calculate the pH of a solution prepared by adding 250 mL of 0.0125 M HNO3to 500.0 mL of 0.0200 M HNO3.6. Calculate the pH of 0.15 M C5HSNHCI. Kp =5.62 x 10 for CSHSN.7. Calculate the pH of 0.25 M KF. K, = 3.53 x 10* for HF.

Acid is defined as a substance that releases hydronium ion when dissolved in water. Acid is…

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Calculate the pH of a solution prepared by adding 250 mL of 0.0125 M HNO3 to 500.0 mL of 0.0200 M HNO3.

Fundamentals Of Analytical Chemistry

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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

8. Products are favored in each of the following reactions.
HNO3(aq) + CN (aq) HCN(aq) + NO3 (aq)
HCN(aq) + OH (aq) H20() + CN (aq)
H20() + CH30 (aq):
=CH3OH(aq) + OH (aq)
Identify the weakest acid and explain your answer.
Identify the strongest base and explain your answer.
9. The salt of a weak acid HA has the formula NaA. The pH of 0.135 M
NaA is 10.7. Calculate the Ka for HA.

5. Calculate the pH of a solution prepared by adding 250 mL of 0.0125 M HNO3
to 500.0 mL of 0.0200 M HNO3.
6. Calculate the pH of 0.15 M C5HSNHCI. Kp =5.62 x 10 for CSHSN.
7. Calculate the pH of 0.25 M KF. K, = 3.53 x 10* for HF.

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