Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 305 mL 0.0409 M 3-(N-Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pK, of MOPS is 7.18. NaOH volume = mL
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- Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 319 mL 0.0439 M 3‑(?N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pKa of MOPS is 7.18. NaOH volume = mLCalculate the volume, in milliliters, 0.170 M NaOH that must be added to 303 mL 0.0471 M 3‑(?N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of7.55. The pKa of MOPS is 7.18.What will be the pH of the buffer solution consisting of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189 mol/L and 109 mL sodium butanoate (CH3CH2CH2COONa) 0.207 mol/L, if 10.9 mL KOH 0.5 mol/L is added?Give an answer to at least 3 decimal places.
- Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 299 mL 0.0611 M 3‑(?‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The p?a of MOPS is 7.18. NaOH volume= mLCalculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid. The Kb for hydrazine is 3.00x10-6. 9.39 3.32 4.80 9.60 4.70 3.22Consider the titration of 100.0 mL of 0.200 mol/L ethanoic acid, HC2H3O2(aq) (Ka = 1.8 x 10-5), by 0.100 mol potassium hydroxide solution. Calculate the pH of the resulting solution when 150.0mL of potassium hydroxide solution has been added?
- In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?Find the pH of a solution produced by the reaction of 250mL 0.1 M NaOH and 150mL 0.03 M acetic CH3COOH note that the pKa of acetic acid is 4.76A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added
- A water sample from a river has a pH of 7. What species make up the carbonate system of this sample? And which ones contribute to the total alkalinity of this same sample?A solution of 0.138 M aspartic acid, the charge neutral form of the amino acid, is titrated with 0.0460 M NaOH . The p?a values for aspartic acid are 1.990 , 3.900 , and 10.002 , corresponding to the α-carboxylic acid group, the β-carboxylic acid group, and the amino group, respectively. Calculate the pH at the first equivalence point of this titrationAn 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?