:The electrolyte solution within the glass electrode (ref) of the pH meter is .a O Dilute KC1 Saturated KCI .b O Dilute HCI .c O .d O Dilute NaCI Concentrated HCI .e
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- A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanationHow to solve for no.1? ps. With solutions. Not graded activity.Please answer subparts d-e. Show solutions. Thanks
- In non-aqueous volumetric methods:I. Carbon dioxide and water is excluded to prevent these from reacting with the sample.II. The temperature is controlled to prevent loss of solvent.III. Samples are usually organic acids and organic bases which are weak electrolytes. a. I & III b. II only c. II & III d. I only e. I, II & IIIFor an experiment, you made a solution that was 0.0100 M acetic acid and 0.1400 M NaCl. a. What is the ionic strength of the solution? b. Without accounting for activities, what is the pH of the solution? c. What are the activity coefficients of all of the relevant species in this system? d. Accounting for activities, what is the pH of the solution? e. What is the percent error incurred by not accounting for the activity coefficients? Please help with dIn non-aqueous volumetric methods:I. Carbon dioxide and water is excluded to prevent these from reacting with the sample.II. The temperature is controlled to prevent loss of solvent.III. Samples are usually organic acids and organic bases which are weak electrolytes. I & III II only II & III I only I, II & III
- The calculated concentration of Ag+(aq) from the student’s data is lower than the actual concentration of the original solution. The student claims that the calculated concentration is too low because some of the AgCl(s) passed through the filter paper. Do you agree or disagree? Justify your answer.Hydrogen H2{"version":"1.1","math":"<math xmlns="http://www.w3.org/1998/Math/MathML"><msub><mi mathvariant="normal">H</mi><mn>2</mn></msub></math>"} is ___________________________ in water. Question options: insoluble soluble and a nonelectrolyte soluble and an electrolyte00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M. Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH. Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL 0.1506 M 0.0753 M 0.0376 M 0.1431 M 0.0526 M
- ignore "solution a & b" partA 4.0520g sample of HCl, specific Gravity 11.18, required 44.15ml of 0.9035M of Sodium Hydroxide in titration, compute for percent purity. Please explain thoroughly. Final answer in percent.Can you please answer sub questions A and B and show all of the steps to the solution please and thank you