5. A common solvent for diluting biochemical samples like the protein you are using in this lab is a buffered 0.05 M Tris solution buffered at pH 7.4 that contains 0.15 M NaCl. Considering your answers to the previous questions, explain why this solvent is suitable for diluting your samples.
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- 4. How many grams of methanesulfonic acid and sodium lactate must be added to 1L of water to produce a solution with pH 3.9 and a total solute concentration of 0.5 mM?1. Calculate the pH of the following solutions: a) 0.1000 M NaOH, b) 0.1000 M CH3COOH (Ka = 1.8x10–5), and c) 0.1000 M NH3 (Kb = 1.8x10–5). 2. Calculate the pH of a solution when 10.00 mL of 0.1000 M NaOH is added to 20.00 mL of 0.1000 M HCl. (SA-SB) 3. Calculate the pH of a solution when 10.00 mL of 0.1000 M NaOH is added to 20.00 mL of 0.1000 M CH3COOH. (SB-WA) 4. Calculate the pH of a solution when 10.00 mL of 0.1000 M NH3 is added to 20.00 mL of 0.1000 M HCl. (WB-SA)14. A so-called PBS buffer (phosphate buffered saline) is prepared by according to the given protocol: ● Prepare 800 mL of distilled water in a suitable container; ● Add 8 g of NaCl to the solution; Add 200 mg of KCl to the solution; Add 1.44 g of Na₂HPO4 to the solution; Add 245 mg of KH₂PO4 to the solution; Adjust solution to desired pH (typically pH ≈ 7.4); and Add distilled water until volume is 1 L. (a) Calculate the pH of the initial solution (before pH is adjusted). (b) How many moles of acid or base are required to adjust the pH to 7.4?
- Using the table of the weak base below, you have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula 1.8 × 10-5 4.38 × 10-4 5.6 x 10-4 3.8 × 10-10 1.7 x 10-9 NH4 CH;NH3* NH3 CH;NH2 C¿H;NH2 CH;NH2 C;H;N Ammonia Methylamine Ethylamine Aniline C¿H§NH3* CH;NH;* C;H;NH+ Pyridine 3. Compute the concentration of the weak base in Molarity. (round off final answer to 4 decimal places)3. The pH of an acid solution is 6.20. Calculate the Ka for the acid. The initial acid concentration is 0.010 M. 4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium? 5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. Calculate the percent ionization of Ammonium hydroxide, NH4OH at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions.…How many moles of sodium acetate should be added to 0.40 mol CH3COOH to make a solution buffering at pH = 4.46 (pKa - 4.76 for CH3COOH)? O 0.4 moles O 0.6 moles O 0.3 moles O 0.2 moles
- Calculate the volume of concentrated ammonia (molecular weight = 17) (PH needed to prepare 100 ml of buffer solution equal to 10.0 if the final concentration of salt is 0.2 molarity. Note that the percentage of concentrated ammonia is 28% * .10-5 x and %3D its density is 0.9 g / mL and dissociation constant 1.8Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Name Formula Kb 1.8 x 10-5 Ammonia Methylamine NH3 CHÍNH, 4.38 x 10-4 C₂H5NH₂ 5.6 x 10-4 Ethylamine Aniline CHẠNH, 3.8 x 10-10 Pyridine CsHsN 1.7 x 10-⁹ 2. Compute for pKb Conjugate Acid NH4+ CH;NH * C₂H5NH3+ CH,NH,* CH,NH*The experimental pH of a 0.25 M solution of potassium hydrogen phosphate, K2HPO4, is 10.25. a. Is the solution acidic, basic, or neutral? B. Write the balanced net ionic equilibrium reaction. Identify the acid, base, conjugate acid, and conjugate base. Write the cquilibrium expression Kb for the reaction. C. Look up the theoretical pKafrom the CRC Handbook. Please give me all questions solution fast
- 2. If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of BaCl2? 3. What is the pH of a solution that is 0.010 F HBr? 4. What is the pH of a solution that is 0.150 F in HBr? (You will need to use the Debye-Huckel equation to answer this.)Calculate the pH of a solution prepared by mixing 0.0870 mol of chloroacetic acid plus 0.0250 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations. The pK, of chloroacetic acid is 2.865. pH = 2.323 Then do the calculation with [HA] and [A-] from Equations 9-21 and 9-22. [HA] = FHA – [H*]+ [OH¯] (9-21) [A] = FA- + [H*] – [OH-] (9-22) 8.54 x103 pH = Incorrect Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00 L: 0.250 mol CICH,CO,H, 0.090 mol CICH,CO, Na, 0.080 mol HNO,, and 0.080 mol Ca(OH),. Ca(OH), provides 2 OH-. pH = 2.865We want to prepare a buffered solution having a pH of 4.97 using concentrated (23.6 M) formic acid (HCOOH) and solid sodium formate (HCOONA). Ką for formic acid is 1.8 x 10-4. Incorrect. Calculate the ratio [HCOO (aq)] / [HCOOH(aq)] in the buffered solution required to achieve a pH of 4.97. [HCOO (aq)] /[HCOOH(aq)] = i 1.68E1 eTextbook and Media Hint Save for Later Attempts: 2 of 3 used Submit Answer