"p" Calculation practice Homework • Answered The acid base indicator phenolphthalein has a Kg = 4.0 × 1071º. what is the pKa for phenolphthalein? Type your numeric answer and submit 9.3 You are incorrect
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- The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)? Show step by step process.A 10.00 mL sample of acetic acid (CH3COOH) and a few drops of phenolphthalein indicator are addedto a conical flask. From burette, 0.75 M NaOH is slowly added. When phenolphthalein indicator turns a lightpink, reading noted was 8.3 ml. Calculate the concentration of acid present in flask. Also write equation.What is pOH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10 Group of answer choices 9.07 4.73 4.93 9.27
- Lactic acid, HC3H5O3, is a monoprotic acid that dissociates in aqueous solution. If a solution containing 0.50 M lactic acid is 1.66 percent dissociated to ionic form, calculate the value of Ka for lactic acid. Include answer to 3 significant figuresIn the video, what is the color of universal indicator in the most basic solution? What is (chemical name and formula) of the chunk of solid stuff added to the solution? What acid is produced when dry ice is added to water? Is this acid produced a weak or strong acid? According to the video, what is the approximate pH of a yellow solution with the universal indicator? Video is https://www.youtube.com/watch?v=iK_CCa5ZMKg&t=1s"M" in .25M represents what? Question 4 options: Concentration None of the above Color pH
- The acid–base indicator bromcresol green is a weak acid.The yellow acid and blue base forms of the indicator arepresent in equal concentrations in a solution when the pHis 4.68. What is the pKa for bromcresol green?Which of the following salts would give you the lowest concentration of sulfate ions in solution if you placed 1 mole of the salt in a liter of water? Question 6 options: A) BaSO4 Ksp= 1.1 x 10-10 B) CaSO4 Ksp= 2.4 x 10-5 C) SrSO4 Ksp= 2.8 x 10-7 D) PbSO4 Ksp= 1.8 x 10-8How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid, HBrO, to form a buffer solution of pH 8.95? The Ka of HOBr is 2.0 × 10–9. Express your answer in moles using at least three significant figures. Do not use scientific notation.
- How many grams of solid potassium hypobromite, KBrO must be added to 500.0 ml of 0.500M hypobromous acid in order to form a buffer with a pH = 8.80?Answer grams of KBrOThe pH of an acetic acid-sodium acetate buffer is 4.50. Calculate the ratio [CH3COO‾]/[CH3COOH]. Refer to Sample Problem 3 for the Ka value.Hint: Let [CH3COO‾]/[CH3COOH] = x. If log x = y, then x = 10y.Data: NaOH added mL pH 2 3.90 4 4.20 6 4.4 8 4.6 10 4.70 12 4.86 14 5.02 16 5.1 18 5.3 20 5.5 22 5.89 24 6.6 24.5 9.9 25 10.88 25.5 11.4 26 11.7 27 11.98 28 12.03 29 12.05 1. determine the pH and volume of NaOH added at the equivalence point. 2. Calculate the Ka for acetic acid. 3. Determine the percent error for the Ka value