Consider a buffer made by adding 55.5 g of (CH3)2NH2I to 250.0 mL of 1.42 M (CH3)2NH (Kb = 5.4 x 10-4) What is the pH of the buffer after 0.300 mol of H* have been added?
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A: The reaction taking place is,
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- A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.In some water softening operations, Mg2+ must be removed from solution along with Ca2+. What is the minimum pH required to lower TOTMg to 10 mg/L as CaCO3 by precipitation of Mg(OH)2(s)?A solution of volume 0.500 L contains 1.68 g NH3 (Kb = 1.8 x 10^-5) and 4.05 g (NH4)2SO4. How many milliliters of 12 M HCI must be added to 0.500 K of the original solution to change its pH to 9.00?
- Tris(hydroxymethyl)aminomethane is a common base used to prepare buffers in biochemistry. Its Kb is 1.2 x 10−6. What would be the pH of the resulting solution if 100.0 mL of 0.05240 M KOH is added to 900.0 mL of the buffer containing 0.01335 M tris (B) and 0.02960 M tris hydrochloride (BH+)?Consider a buffer made by adding 57.9 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x 10⁻⁴) What is the pH of the buffer after 0.300 mol of H⁺ have been added?What volume in mL of 0.2572 M NaOH must be added to 500.0 mL of 0.1000 M chlorous acid (HClO2, Ka = 1.10 x 10–2) to produce a buffer solution with a pH of 2.25?
- Consider a buffer made by adding 57.9 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x 10⁻⁴) What is the pH of the buffer after 0.120 mol of OH⁻ have been added?A solution is prepared by dissolving 1.800 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.180 M solution of acetic acid. The Ka of acetic acid is 1.8 x 10-5. What is the pH of the solution?A microbiologist is preparing a medium on which to cultureE. colibacteria. She buffers the medium at pH 7.00 to minimize the effect of acid-producing fermentation. What volumes ofequimolar aqueous solutions of K₂HPO₄and KH₂PO₄must shecombine to make 100. mL of the pH 7.00 buffer?
- At 25°C, 50.0 mL of 0.50 M NaOH(aq) is added to a 250 mL aqueous solution containing 0.30 M NH3 and0.36 M NH4 Cl. What is the pH of the solution after the addition of the base? Assume that volumes areadditive. Kb of NH3 = 1.8 x 10−5Consider a buffer made by adding 42.3 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x 10⁻⁴) What is the pH of this buffer?A sample of 0.1687 g of an unknown monoprotic acid wasdissolved in 25.0 mL of water and titrated with 0.1150 MNaOH. The acid required 15.5 mL of base to reach theequivalence point. (a) What is the molar mass of the acid?(b) After 7.25 mL of base had been added in the titration,the pH was found to be 2.85. What is the Ka for the unknownacid?