[4} What is the pH of the solution in the flask after 25.00 mL of 0.110 M NAOH has been added to 50.00 mL of 0.108 M HCIO solution using phenolphthalein as an indicator? The K, of HCIO is 3.0x10 at 25°C.
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![[4} What is the pH of the solution in the flask after 25.00 mL of 0.110 M NAOH has been added to 50.00 mL of 0.108 M HCIO
solution using phenolphthalein as an indicator? The K, of HCIO is 3.0x10 at 25°C.
[5] On the back of the quiz, derive the acıd form of the Henderson-Hasselbalch Equation (above) as was done in class.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5b71dfa4-9e2c-4066-8311-8d9bf43b1c6f%2F84c9c628-ec5b-4658-b575-ac37fbd9d1d5%2Fb0bnmxr_processed.jpeg&w=3840&q=75)
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- You were asked to estimate the pH of a 15mL of 0.09N of HCl when 16.9mL of 0.085N NaOH is added to a solution. Your supervisor informed you that she added 100 mL of diluent. With your computed pH and Phenolphthalein as the indicator [pH range: 8.00 – 10.00], would you expect a color change? Yes or No?How will you prepare a pH 4.50 acetic acid-acetate buffer such that when1.00 mL of 10 M NaOH is added to 100.00 mL of this buffer, the resulting pHwill be raised by exactly 1 pH unit? Show calculations for the concentrations(in 3 decimal places) of the components that must be present in the bufferas well as the volumes of 1 M acetic acid and 1 M sodium acetate that needto be mixed and diluted to 100.00 mL to prepare the buffer. (There is nospecific final buffer concentration required here. You can verify your answersby using the Virtual Lab).If 250.0 mL of 9.84 x 10-4 M HNO3 is mixed with 150.0 mL of 1.18 x 10-5 M HBr, what is the resulting pH?
- In the lab, you have access to the following solutions: 0.500 M ammonia, 0.500 M acetic acid, 2.00 M nitric acid, and 2.00 M sodium hydroxide. How would you prepare 500.0 mL of a buffer of pH = 5.00? Assume volumes are additive.When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?Magnesium carbonate is slightly soluble in water. The Ksp for MgCO3 is 3.5 x 10-8. The carbonate ion being a conjugate base may form the bicarbonate ion (HCO3-) and carbonic acid (H2CO3) in solution. Which of the following represents the correct mass balance equation at a pH of 7.5 for this system?
- You are to prepare 100. mL of an acetate buffer of pH 5.00 using 1.0 M acetic acid (CH3CO2H, also written as HC2H3O2) and solid sodium acetate (NaC2H3O2). To prepare for the investigation, complete the following calculations. The pKa for HC2H3O2 is 4.74. The Henderson-Hasselbach equation is pH = pKa + log ([conjugate base]/[acid]) (a) What ratio of [NaC2H3O2] to [CH3CO2H] is required for a pH = 5.00? (b) You will want the concentrations relatively dilute, so use an acid concentration of 0.10 M. What volume of 1.0 M CH3CO2H would be needed to prepare 100. mL of buffer with the desired concentration of 0.10 M? Use M1V1 = M2V2 (c) Use the ratio from (a) and the concentration desired (discussed in (b)) to calculate how many grams of NaC2H3O2 · 3 H2O would be needed to prepare 100. mL of buffer if the acid concentration is 0.10 M?A professor prepares a buffer solution that they need for the purification of protein from human cell lysates. They did mix weak acid and conjugate base and obtained the initial solution, which is characterised by these parameters. Final volume: 200mltotal buffer compound concentration: 150mMIntitial concentration weak acid: 0.03MInitial concentration conjugate base: 0.12MInitial pH 6.9buffer compound pka 6.3An enzyme-catalyzed reaction is carried out in a 250 mL solution containing 0.1M TRIS buffer. The pH of the reaction mixture at the start was 7.8. As a result of the reaction, 0.003mol of H+ was produced. What is the ratio of TRIS base to TRIS acid at the start of the experiment? What is the ratio at the end of the experiment? What is the final pH?
- If the actual mass of a base used (sodium citrate dihydrate) in a buffer solution is 1.5 g, and the concentration of the acid used (5 mL, ammonium citrate) is 2 M, with a Ka of 4.06E-7, what is the concentration of this base (in M) in this buffer solution?If 40.0 mL of formic acid with a concentration of 0.300 M and a Ka of (2.258x10^-5) is titrated with 0.300 M lithium hydroxide what is the pH of the solution after 20.00 ml of base has been added? Note: Your answer is assumed to be reduced to the highest power possible."You are asked to estimate the pH of a 15mL of 0.09 N of HCl when 16.9mL of 0.085 N NaOH is added to the solution. Your supersaver informed you that she added 100mL of diluent."
