H2PO4- + H2O <=====> HPO4-2 + H3O+ 1. Using 0.1 M phosphate buffer, pH 7.2, prepare 25mL each of the buffer solutions with the following concentrations at pH 7.2: a. 0.005 M b. 0.05 M c. 0.10 M
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H2PO4- + H2O <=====> HPO4-2 + H3O+
1. Using 0.1 M phosphate buffer, pH 7.2, prepare 25mL each of the buffer solutions with the following concentrations at pH 7.2:
a. 0.005 M
b. 0.05 M
c. 0.10 M
Step by step
Solved in 2 steps with 1 images
- For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surelyans asap In the use of EDTA as the complexometric titrant, at what pH value/s does Y4- become a major component of solutions? -At pH 1 -At pH 7 -At pH values lower than 10 -At pH values greater than 10Utilize the systematic treatment to determine the concentrations of all species present in a solution of: 1.) 0.35 M CaF in H2O 2.) saturated PbSO4 buffered at pH 7 3.) 0.05 M KC2O4 in H2O Please show COMPLETE solution
- 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?The concentration of Cl– in a 300.0-mL sample of water drawn from a fresh water acquifer suffering from encroachment of sea water, was determined by titrating with 0.0516 M Hg(NO3)2. The sample was acidified and titrated to the diphenylcarbazone end point, requiring 6.18 mL of the titrant. Report the concentration of Cl–in parts per millionThe pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.
- The protein content of wheat flour can be determined reasonably accurately by multiplying the percentage of nitrogen present by 5.7. A 2.06-g sample of flour was taken through a Kjeldahl procedure and the ammonia produced was distilled into a boric acid solution. If this solution required 34.70 mL of 0.174 N HCl for titration to the methyl red end point, what is the a) % Nitrogen and b) % protein in the flour? (Use 1:1 stoich ratio between N and HCl)When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?A 0.3606-g of a weak monoprotic was dissolved in water and then titrated with 0.1040 N KOH solution. A total of 28.39 mL of the base was consumed in the titration to reach the endpoint. What is the equivalent weight of the acid? If the pH at ½ EP is 4.194, what is the Ka of the acid?
- The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.a. Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. b. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.The Tris buffer system is commonly used in biochemistry as its pKa of 8.1 allows it to buffer close to physiological pH. (CH2OH)3CNH2 + H+ Û (CH2OH)3CNH3+ What concentrations of Tris and Tris H+ are obtained in a 200 mL solution at pH 8.20 containing 6.1g of Tris? The molecular mass of Tris is 121.1 gmol-1 Please do this step by step thank you!John wanted to determine the protein content of his blood. To do so, he obtained 1.00 mLof blood, and diluted it to 10.00 mL. From that solution, he subjected 1.00 mL to Kjeldahl analysis. After digestion, the liberated NH3 was distilled in a flask containing exactly 25.00 mL of 0.0150 M H3BO3. Titration requires 5.85 mL of standard 0.0150 M NaOH to reach the desired endpoint. If a typical blood sample contains 15.45 g N per 100 g protein, calculatethe protein content (in g/mL) in the sample of John’s blood.
