Starting with 2.0 g of hand sanitizer in 10 mL of methanol (density of methanol = 0.791 g/mL), the Karl Fischer titrator returned a water content of 4.0%. What was the original water concentration in the hand sanitizer?
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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)While making a stock solution of NaSCN using 0.8 g of NaSCN in a 10 mL volumetric flask. 750 microliters of this solution were added to a 3500-microliter cuvette. What is the initial concentration of NaSCN in the cuvette? A. 0.21 M B. 13.18 M C. 2.82 M A. 1.07 M
- Suppose you prepared a stock solution of Ca(OH)2 by dissolving 0.6580 g (weight obtained from digital balance) of Ca(OH)2 in a 50-mL volumetric flask. a) Calculate the molarity of the Ca(OH)2 stock solution. M b) Calculate the % inherent error in the Ca(OH)2 solution c) Calculate the % (m/v) of the Ca(OH)2 stock solution % d) Calculate the absolute error (in molarity) for the Ca(OH)2 solution.1. What is the concentration of the titrant in Normality? 2. What is the mEq of KOH in mg/gram? 3. Find the acid value of the sample 4. Find the saponification Value of the sample5. Seawater is titrated with 0.2 M of NaOH. The salinity of the seawater is 3.25% and the density of the seawater is 1.024 g/mL. The titration volume is 25.5 mL. Find the number of moles of Na+ the ion exchange column absorbs from the seawater
- 1)A bottle of concentrated aqueous sulfuric acid, labeled 95.00 wt% H2SO4, has a concentration of 16.5 M. Calculate the density of 95.00 wt% H2SO4. 2)Ascorbic acid in 5 vitamin C tablets was measured by a titration against (100 ± 0.002 M) NaOH solution. It required 10.00 ± 0.05 mL NaOH solution to reach the equivalent point. What is the average quantity of ascorbic acid per vitamin tablet?Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant. What substance served as the primary standard?Which served as the indicator in the titration?What is the color at the end point?What is the concentration of the titrant?What is the molar concentration of the acetic acid solution?A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible.What is the MW of calcium carbonate?102 g/mol98 g/mL100 g/mL100 g/molWhat is the molar concentration of the standardized EDTA solution?0.08m0.8M0.08N0.08MHow many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?0.18250.18521.8251.1852
- C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the MW of calcium carbonate? (use C1 as reference)* 102 g/mol 98 g/mL 100 g/mL 100 g/mol What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852You used the back-titration method to experimentally determine the amount of CaCO3 in an Ultra Strength Tums antacid tablet. You calculated that you used 21.5 mmol HCl to complete the titration of a 2.139 g Tums tablet. What is the mass (in mg) of the active ingredient in the Tums tablet? (CaCO3 = 100.1 g/mol)A 24.8mL sample of vegetable juice is titrated with 15.65mL of NaOH solution. The molar concentration of the NaOH is .106 M. The molar mass of citric acid is 192.12 g-mol-1. Express all with three significant figures. 1. If the label on the bottle lists the citric acid content as 1 g per serving with a serving size of 240 mL determine the percent error in the titration results. express finale answer with 2 sig figs.
