Estimate (to ±0.1) pH values of the following solutions:
1. 0.25 M lactic acid
2. 0.025 M methylamine
3. 0.25 M potassium carbonate
4. 0.08 M methylammonium chloride
Estimate (to ±0.1) pH values of the following solutions: 1. 0.25 M lactic acid 2. 0.025...
Estimate to ±0.1 the pH value of the following solutions: 1. 0.043 M sodium hydrogen carbonate 2. 0.017 M sodium hydrogen tartrate Blood pH is regulated to stay within the narrow range of 7.35 to 7.45, making it slightly basic. Which form of the following molecules is predominant at pH 7.4 (draw formula in ChemDraw or ChemSketch with appropriate protons shown): 1. Pyridine 2. Ethylamine 3. Acetic acid 4. Citric acid 5. Ibuprofen (pKa =4.91) 6. Glycine 7. Amphetamine (pKa...
A) Calculate the pH of the following simple solutions: 0.08 M HCl 0.25 M KOH 0.08 M HCl + 0.25 M KOH Is solution “c” a buffer? Why or why not? B) Suppose you dissolve 0.1 moles of formic acid in 1 water. What are all of the molecules and ions you would expect to find? Which one of the above will be found in the greatest total amount? Which of the above will be found in very small amounts?...
2. (a) Determine the pH of 0.10 M lactic acid (HC3HSO3) (b) What is the pH of a buffer that is 0.12 M. lactic acid and 0.10 M sodium lactate (NaC3H5O3)? For lactic acid. Ka = 1.4 x 10-4. (10)
1. Calculate pH and % ionization of 0.25 M Naco (Ka (HCO2H) 1.8 x 10") 2- Calculate the pH of: a) 0.35 M HNO b) 0.15 M Sr(O)2 c) 0.08 M Ba(CIO4)2 3- Calculate the pH of 0.375 L buffer solution made of a 0.18 M Acetic acid HC2H:02(Ka 1.8x 10) and a 0.134 M Potassium acetate KC2Hs02 (do not use more than 3 digits beyond the decimal point) a) before adding anything b) after adding 0.010 mol Ba(OH)2 c)...
1. Complete an ICE table and calculate the pH for the following solutions. a. 0.50 M HC,H,O2 (benzoic acid, Ka = 6.5 x 10) b. 0.10 M CH3NH2 (methylamine, Kb 4.4 x 10) c. 0.50 M NaC7H,O2 (Sodium benzoate) d. 0.10 M CH3NH3CI (methylammonium choride) e. 0.10 M Na2SO4 (sodium sulfate; Ka2 for H2SO4 0.012) 2. What is an amphoteric species? Provide an example of an amphoteric species and write balanced equations that show why it's amphoteric.
Determine the pH to two deci al places of the following solutions. A table of p a values can be o n ere the 5% approximation svaid use the assumption to compute h 4.18x10 1 M hypochlorous acid ???? ??. Tries 1/3????? 8.91×10-2 M methylammonium chloride ???? Tries 0/3 9.59x101 M sodium lactate ???? Tries 0/3 2.96×10-3 M sodium sulfite ???? Tries 0/3
Which one of the following solutions has the lowest pH? A. a 0.1 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) B. a 0.1 M solution of ammonium chloride, NH4Cl(s) (Ka (NH4+) = 5.6 x 10-10) C. a 0.01 M solution of acetic acid, CH3COOH (Ka = 1.8 x 10-5) D. a 0.01 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) E. a 0.1 M solution of acetic acid, CH3COOH (Ka = 1.8 x...
17;1.1 Which of the following aqueous solutions are good buffer systems? 0.25 M ammonia +0.33 M calcium hydroxide 0.15 M barium hydroxide +0.23 M barium chloride D 0.35 M barium chloride +0.20 M potassium chloride O0.13 M hypochlorous acid + 0.16 M potassium hypochlorite @0.28 M hydrobromic acid +0.22 M potassium bromide Submlt Answer Retry Entire Group 3 more group attempts rema
Given stocks of 1 M Lactic Acid (pKa 3.86) at pH 3.5, 2 M naOH, 2 M HCl and water: how would you prepare 4 liters of 0.05 M Lactic Acid at pH 3.25? Give 2 M Tris, pH 7.1 (pKa 8.0), 5 M NaOH, 5 M HCl, and water: how would you prepare 2 L of 0.2 M Tris, pH 7.4?
Determine the pH (to two decimal places) of the following solutions. A table of pKa values can be found here. If the 5% approximation is valid, use the assumption to compute pH. 6.80×10-3 M butanoic acid Tries 0/13 9.74×10-1 M formic acid Tries 0/13 8.47×10-3 M methylamine Tries 0/13 6.59×10-3 M triethylamine