What is the importance of calibrating pH electrode and weighing balance during buffer preparation? What will happen if either of them is uncalibrated? Which will result to bigger error?
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What is the importance of calibrating pH electrode and weighing balance during buffer preparation? What will happen if either of them is uncalibrated? Which will result to bigger error?
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- The course is specifically quantitative analysis, I figured that would just fall under chemistry. The issue I'm having with this one is that I have absolutely no idea how to even begin. I figure benzoic acid wouldn't affect the pH of NaOH that much since it's a weak acid and NaOH is a strong base, but I don't think it'd be right to just take the pH using solely the concentration of NaOH. What approach should I take to solve this? 220 mL of 0.03 M NaOH were added to 200 mL of 0.03 M benzoic acid (pKa = 4.2). What is the pH of the resulting solution?Buffers remoteWhich statement is NOT correct? pH meter should always be standardized before using to make sure that your readings are accurate and repeatable. The electrode tips should never touch the bottom or sides of a beaker. When finished using the pH meter, rinse the electrode and place it in the pH 7 buffer solution on standby. One buffer solution is enough to standardize a pH meter before using.
- topic: Proper Use and Calibration of the pH meter Why is it necessary to rinse the pH electrode with distilled water every after pH readings? explain pleaseThe student added universal indicator to the alkali solution at the start of the experiment. The indicator changed colour when the acid was added to the alkali. Explain how the student used this information and the pH scale to explain that this is a neutralisation reaction.1. How does calculation of the electrode potential of the system at the equivalence point differ from that for any other point of an oxidation/reduction titration?
- 1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/LHow is coulometric titration done? Explain step by step.Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. adding titrant past the color change of the analyte solution recording the molarity of titrant as 0.1 M rather than its actual value of 0.01 M spilling some analyte out of the flask during the titration starting the titration with air bubbles in the buret filling the buret above the 0.0 mL volume mark Answer Bank no effect too low too high 7
- Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. ANSWER BANK: Too low, No effect OR Too high adding titrant past the color change of the analyte solutionrecording the molarity of titrant as 0.1 M rather than its actual value of 0.01 Mspilling some analyte out of the flask during the titrationstarting the titration with air bubbles in the buretfilling the buret above the 0.0 mL volume markFor indicator electrodes, which statements are true?I Indicator electrodes are made from relatively inert metals.II Indicator electrodes work best when the electrode surface is large and clean.III Platinum is a common indicator electrode.IV Platinum electrodes are more inert than gold electrodes. A. I, III, and IV B. I, II, and III C. I, II, III, and IV D. II and III E. I, II, and IVyour EDTA stock solution has an initial pH of 8.0. If you dilute the stock solution with water, do you expect the pH to change?