hello, i need help with this question. An aqueous solution of a monoprotic acid HA (Ka = 3.10×10-1) has a pH of 4.66. 1a) What is the molarity of the solution? (i.e. [HA]+[A-].)

what is the pH of a 0.250 M monoprotic weak acid HA (Ka = 1.54 × 10-6)

1.) In a 0.100M aqueous solution of a weak acid, the acid is 3.7% dissociated. What is the Ka for this acid?   2.) What is the pH of a 0.010M solution of pyridine, C2H5N, a weak base? It's Kb is 1.5x10-9.   3.) Calculate the pH and percent ionization of a 15.0 M solution of a weak base. (pKa=9.26)   SHOW ALL WORK!!

а A solution is prepared at 25 °C that is initially 0.51M in chloroacetic acid (HCH2CICO₂), a weak acid with K = 1.3×10 chloroacetate (NaCH,CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH ☐ X

Calculate the pH of a solution that contains 0.00415 M HI and 0.400 M benzoic acid. (Ka for benzoic acid is 6.5×10−5)

What is the pH of a solution made by adding 0.65 mol of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution?  (Ka = 1.8 x 10-5)   Group of answer choices 8.92 5.08 4.74 4.40

This question has two parts. Part-I (a) Calculate the pH of a 0.20 M HF solution. The Ka of HF is 6.8*10-4. Show the ICE table and all calculations.   Part-II (b) Calculate the pH of a solution containing both 0.20 M HF and 0.10 M HCl? The Ka of HF is 6.8*10-4. Show the ICE table and all calculations.

25.00 mL of a 0.22M C6H5COOH(KA = 6.3x10-5) is titrated with a 0.15 M NAOH solution. What is the pH of the solution after 23.4 mL of NaOH is added? A Moving to another question will save this response. «< Question 3 of 7 24:01 hulu & 5 Σ

A student is given a weak monoprotic acid "HA" that has a Ka = 0.00008885. What is the % ionization of a 0.19 molar aqueous solution of HA? (Enter your number with two significant figures and DO NOT include the percent sign in your answer)

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