Problems to solve pH = pka + log [A] [HA] 1. The pKa of acetic acid is 4.8. If you mix 100 ml of 0.1 M acetic acid with 1 ml of 0.1 M sodium acetate, what will be the pH of the resulting solution? 2. The pKa of lactic acid is 3.9. In a solution of lactic acid/lactate at pH = 4.9, what is the ratio of lactic acid/lactate?
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- You prepare a buffer solution from 10.0 mL of 0.100M MOPS (3‑morpholinopropane‑1‑sulfonic acid) and 10.0 mL of 0.075 M NaOH. Next, you add 1.00 mL of 4.15×10−4 M lidocaine to this mixture. Denoting lidocaine as L, calculate the fraction of lidocaine present in the form LH+. MOPS Ka = 6.3 * 10^-8 Lidocaine Kb = 8.7 * 10^-7 ( Please type answer note write by hend )How many grams of NaOH are needed to make 100.0 mL of a 0.130 M acetic acid/acetate buffer pH 5.20 from 1.00M acetic acid and solid NaOH? pka for acetic acid is 4.74 and molecular weight for NaOH is 40.00 g/mol I know the answer is 0.386 grams, please show workOne of the components in TAE is 0.5 M EDTA. Answer the following: a. How much EDTA is needed to prepare 100 ml of 0.5 M EDTA? EDTA MW = 372.2 g/mole b. As EDTA dissolves in water, the [H+] will increase (note that full name of EDTAincludes "acetate"). To achieve a pH = 8.0, would you need to add HCl or NaOH? c) When you make your agarose gel, you will need to make 50 ml of 1% (w/v) agarose in 1X TAE. How much agarose is needed to make this solution?
- Question. An aqueous solution of cysteine is acidified to pH 1.5 and titrated with 0.1M NaOH to a pH of 12.8. A. How many distinct equivalent points will be observed on the pH titration curve? B. What is the pH at the first equivalence point? C. What is the pH at the isoelectric point (pI)?A 25.0 mL sample of 0.250 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) is titrated with 0.250 M NaOH solution. Calculate the pH after the following volumes of base have been added. a. 35.0 mL PLEASE SHOW ALL WORKAmmonium hexachloroplatinate(IV), (NH4)2(PtCl6), is one of the few sparingly soluble ammonium salts. Its Ksp at 20°C is 5.6 × 10-6. Compute its solubility in grams per liter of solution.
- Find [PbCl2] in a saturated solution of PbCl2. Ksp = 1.7 x 10-5.A certain organic monoacidic base with an ionization constant of 2.0 E -8 serves as an inidicator in a neutralization titration. An intermediate shade of color is obtained at pH=6. What percentage of the indicator has been converted to the ions at this point? Answer: 67%2. Calculate the solubility of silver acetate, AgCH3COO (s), in solutions buffered at pH = 2.00, 4.00, 6.00, 8.00, and 10.00 at 25◦ C. Take the value of Ksp for AgCH3 COO (s) to be 1.9 × 10−3 M2 at this temperature. Ka = 1.8 * 10^ -5
- The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4 (pKa1 =2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molarsolubility of Mg3(AsO4)2 in water. (b) Calculate the pH of asaturated solution of Mg3(AsO4)2 in water.Problem Solving. Solve the following problems, use GRESA format in answering A mixture of 0.15 M acetic acid and 0.34 sodium acetate is given. Calculate the pH of the medium if the pKa of the acetic acid is 4. 87.You wish to prepare a 0.0125 M buffer with a pH of 5.34. If the pKA of DOMINIC ACID is 5.74, what ratio of DOMINATE/DOMINIC ACID must you use? .72 The final buffer volume must be provided in order to determine the correct ratio. 0.40 2.5 0.28