The Ka of propanoic acid (C2H5COOH) is 1.34×10-5. Calculate the pH of the solution and the concentrations of C2H5COOH and C2H5COO- in a 0.161 M propanoic acid solution at equilibrium. pH=? [C2H5COOH]= ?M

Each of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are monoprotic, meaning that each acid molecule gives up one H+. The pH of each solution is as indicated.  Flask A: pH=1.1  Flask B: pH=2.4  Flask C pH= 2.9 Flask D: pH=5.1  How much strong base is required to neutralize the initial amount of acid? A. All four solutions will require the same amount of base because they all contain acid of the same concentration B. The solution of pH=1.1 will require the most base since it is the strongest acid and has the highest concentration of H+ C. Neither (A) nor (B) is correct.

Determine the [OH-], pH, and pOH of a solution with a [H*] of 0.014 M at 25 °C. [OH-] = M pH = pOH = Determine the [H*), pH, and pOH of a solution with an [OH] of 8.4 x 10-9 M at 25 °C. [H*] = M pH = pOH = Determine the [H*], OH], and pOH of a solution with a pH of 13.05 at 25 °C. [H*] = M [OH¯] = pOH = Determine the [H*], OH], and pH of a solution with a pOH of 13.25 at 25 °C. [H*] = M [OH-] = M pH =

Use the References to access important The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.58 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.007, the hydrogen ion concentration is mol/L.

3. Suppose 10-6 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This gives (H°] = (10-6 mol)/(1000 L) = 10-9 M. Finally, the pH is calculated: pH = -logro[H*]= -log-o{10 °) = 9.0, which corresponds to an alkaline solution! What is wrong? %3D %3D !! !3! 4. Calculate the pH of a 0.15 M solution of acetic acid, CH;COOH (K. = 1.8 x 109).

O ACIDS AND BASES Calculating the pH of a weak base solution 0/3 The base protonation constant ₂ of trimethylamine ((CH³)²N) ¡S 6.31×10¯³. Calculate the pH of a 0.27 M solution of trimethylamine at 25 °C. Round your answer to 1 decimal place. pH = 0 X

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Consider the following data on some weak acids and weak bases: acid base Ka name formula name formula HNO, 4.5 x 10 CgH;NH2|4.3 × 10 - 10 -4 nitrous acid aniline 4 -8 hydrofluoric acid HF 6.8 × 10 hydroxylamine HONH, 1.1 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M HONH3CI choose one v 0.1 M Nal choose one v 0.1 M KNO2 choose onev 0.1 M NaF choose one v

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Which one of the following correctly shows the weak acid equilibrium for trichloroacetic acid, CCI,COOH? A) CCI,COOH (aq)= CC,Co (aq) + ОН (аq) в) ССІ СООН (аq) + н.о () — CC,COOH, (aq) + OH (aq) С) CI СООH (aq) + Н,О (1) CCI,CoO (aq) + H,0* (aq) D) CCI,COOH (aq) + H,O (1) = CC,CO(OH), (aq) + H* (aq)