If you pipet too much volume for your total hardness titration, but carry out the calcium only titration correctly, how will that change your results? Be specific.
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If you pipet too much volume for your total hardness titration, but carry out the calcium only titration correctly, how will that change your results? Be specific.
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- Topic: Standardization of acid and base with back titration Note: Include up to 4 decimal places Kindly explain the process Thank you!If 0.18 mL was used in the blank titration to achieve the same end-point color in the previous question, what is the correct total hardness of the sample? (Picture given is the previous question)Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint
- The color change at the endpoint should persist for 30 seconds. Explain why the time lapse is a good titration technique.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?please just send me a paper solution ASAP please paper solution only
- 5. Please Double check solution. Last 2 solutions have been completely wrong.Hi I am having trouble finishing and finding the rest of the data for my Titration lab. I've already imputed the given data and just need to find the rest of the excel boxes using those data, thank you.1. Prepare 50-mL of a 50 mM H,PO, solution in a 50-ml conical tube. Molar mass of NaH2PO4 H2O used is 138 moles 2. Check the pH of this solution and record. 3. A5 M NAOH solution has been provided. 4. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. 5. Add 205 µl of 5M NaOH into the 50 mM H2PO4 solution. Check the pH and record. 6. Add 205 µL more of 5M NaOH into the 50 mM H2PO, solution. Check the pH and record. 7. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. Complete the following table "predicted pH." Please show all work on a separate sheet of paper and attach. Note that the pK, of H2PO, is 7.2. What would be the predicted pH's? Would they be similar to the actual pH's from procedure? After 45 µl of 5 | After 205 µl more of 5M NaOH Original After 205 µl more After 45 µl more solution M NaOH of 5M NaOH of 5 M NaOH Actual pH 4.30 6.05 6.90 11.01 11.29 Predicted pH
- Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. Consider that the burette was completely filled to the 0 mL mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 21.2 mL C. 21.3 mL D. 22.7 mL 2. What is the unknown weight (grams) in the problem? Your Answer:which of the 6 tests are you doing if you mix two solutions together and a precipitate occurs? Color, flame Tex, acidity Test, solubility ,complex ion formation, gas producing reaction Make a statement of the test that you would like to run first during the investigation and why. A flow chart of your expected results. Safety concerns? A flow chart of the actual results. Make a table summarizing the conclusions (identity chemicals in bottles A-F). Provide brief justificationFor your fine titrations, after reaching the x-1 mL mark from your rough titration, you should add EDTA in 1 mL increments until you reach the endpoint. True False