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Q: An unknown sample containing mixed alkali (NaOH, NaHCO3, or Na,CO3) was analyzed using the double…
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Q: An unknown sample containing mixed alkali (NaOH, NaHCO3, or Na2CO3) was analyzed using t double…
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Q: Given NaOH pellet and water, write down the procedure to make a concentration gradient of 0, 0.1,…
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In RPLC, The retention of a basic analyte in RPLC decreases as the mobile phase pH increases. True or False?
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- Three-point calibration was not performed on the pH meter prior to titration. Is there a positive error, negative error, no effect, or error could not be determined In terms of the Computed pKa of the unknown weak acid?Back titration is usually required when none of the choices the standard solution is volatile. the analyte reacts very slowly with the standard solution. with weak acid - weak base titration reactions. dealing all of the choicesUsing the letters on the image, identify each component of the titration set-up. Buret clamped to a ring stand with a beaker underneath. The letter A appears at the top of the buret, the letter B appears midway down the buret, the letter C appears at the bottom of the buret, the letter D appears next to the beaker, and the letter E appears on the other side of the buret, near the ring stand.
- 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?What is the effect of buffer additives (organic acids) on the enhancement factor?Before running a titration, you calculate the expected endpoint. However, when performing the experiment, you pass the expected endpoint with no visible color change. What is the most likely problem with the titration set-up? Select one: There was an air bubble in the buret tip. The buret tip is leaking titrant into the analyte. There is not enough indicator in the analyte. The analyte solution is being stirred too quickly.
- The standardization of same titrant during the determination of BOD5 of water sample was done separately for Day 1 and Day 5. Upon standardization, it turned out that the concentration of the titrant in Day 1 is higher than the concentration of the same batch of titrant in Day 5. How would you explain this discrepancy? (A) There were bubbles at the tip of the burette during titration. (B) Too much starch indicator was added in the conical flask. Sulfuric acid was added first before potassium iodide. (D) The water used to prepare the Na₂S₂O3 solution was not boiled resulting to proliferation of bacteria.Given NaOH pellet and water, write down the procedure to make a concentration gradient of 0, 0.1, 0.2, 0.4, 0.8, 1.6 mM (1mL each).Calculate the average concentration of Vitamin C in each sample
- An analyte has an Rf value of 0. 75 What does that indicate about the solubility of the analyte in the mobile phase as compared to the stationary phase?You are given 2 ml of a stock solution of phenol red at a concentration of 258 mg/ml and 20 ml of 0.5 potassium phosphate buffer pH 7. You need 100 ml of a solution containing 50 mM potassium phosphate buffer pH 7 and 87 ug/ml phenol red to do a spectrophotometric analysis. How would you make this new solution?Chemistry Laboratory - Determination of Total Water Hardness by Compleximetric Titration