Reaction: 2HCI + Ca(OH)2 →2H20 + CaCl2 Initial Burette Volume of 0.O5M HCI Volume of saturated calcium Final Burette Volume of HCI hydroxide solution 0.019 L 0.006 L 0.015 L Analysis 1. Calculate the volume and mols of HCl required to reach the end point. Volume (0.015L) - (0.006L) = 0.009 L Molarity = 0.05 M = 0.05 mol/L Number of moles of HCI (0.05mol/L) (0.009L) = 0.00045 mol 2. Use mols of HCl to determine the mols of calcium hydroxide.
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- 5.00 mL of stock solution is diluted to 25.00 mL, producing solution ALPHA. 10.00 mL of solution ALPHA is diluted to 25.00 mL, resulting in solution BETA. 10.00 mL of solution BETA is then diluted to 25.00 mL, producing solution GAMMA. dilution factor for ALPHA from stock solution = 0.167 dilution factor for BETA from ALPHA solution = 0.0476 part c and d?The data below was obtained with a Cl- ISE to prepare a plot of mV vs. log[Cl-]. Assume the unknown saltwater solution was diluted as in the procedure before being measured. What is the ppm Cl- of the undiluted unknown solution? Cl- Concentration (ppm) Potential (mV) 10 160 100 94 1000 40 Diluted Unknown Saltwater 132You are given a container with Na3PO3 that is reportedly contaminated. You are asked by your supervisor to determine the percent purity of that sample in order to know the next measures to be taken by the plant. The following are the procedures that you need to do: a. Dissolve sample weighing 1 g in 35 mL water. b. Prepare solution with 45 mL 3% w/v HgCl2, 30 mL 10% w/v C2H3NaO2 and 10 mL CH3COOH. c. Digest sample then filter then rinse the precipitate that weighs 0.2857 g. d. Compute for the % purity.
- A 100 ml bottle of metronidazole 100 mg/ml suspension is available in your pharmacy. Calculate the volume of this suspension needed to be diluted with cherry syrup to prepare 60 ml of a 4% metronidazole suspension. 1 ml of a 1:1000 epinephrine injection was mixed with 20 ml of 1% lidocaine injection. Calculate the new ratio strength of epinephrine in the admixture. (IGNORE ANY VOLUME CHANGES AFTER ADMIXTURE) Instead of preparing 4 grams of tetracaine hydrochloride 4% gel an 8% gel was compounded by mistake. How many grams of the 8% gel and gel base must be mixed to get 4 grams of a 4% gel? How many milliliters of 70% ethanol and 20% ethanol must be mixed to prepare 500 ml of 30% ethanol? A diphenhydramine elixir contains 12.5 mg drug in one teaspoon. The volume of oral vehicle that is to be added to 100 ml of this elixir to reduce its strength by one half its original strength is; 6. 90 capsules of Liothyronine (T3) 15 micrograms are to be prepared. The formula calls for a 1:10000…Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9 How many millimoles of Ba(NO3)2 are needed to completely react with NaIO3? 500 mmol 250 mmol 25 mmol 12.5 mmol What is the concentration of the excess reagent? 0.1125 M 0.3219 M 0.1195 M 0.2375 M What is the molar solubility of Ba(IO3)2 in this solution? 04x10^-5 M 07x10^-5 M 15x10^-5 M 30x10^-5 M
- To a 0.5 g sample of impure NaCl are added 0.784 g of pure AgNO3 (MW = 169.88) crystal. This is in excess of the amount required to ppt. All the Cl as AgCl. After dissolving and filtering out the pptd. AgCl, the filtrate requires 25.50 ml of 0.028M KCNS. What is the percentage of NaCl (MW=58.44) in the sample? A. 55.40 % B. 50.10% C. 45.60% D. 100%A 1.000-gram sample of NaOH (39.997 g/mol) which has been exposed to the air for some time (NaOH will adsorb water and CO2 from the ambient air) is dissolved in water and then diluted to 500.00 mL. 100.0 mL of this solution required 38.60 mL of 0.1062 M HCl to be titrated to the endpoint (~pH 3). A second 100.00 mL portion is treated with excess BaCl2 and then diluted to 250 mL and filtered. 200 mL of the filtrate required 29.62 mL of HCl to titrate to the (~pH 8-9) endpoint. Calculate the mass percentage of NaOH and Na2CO3 (105.9898 g/mol) in the original sample. The adsorbed CO2 is converted to Na2CO3. The Ksp for BaCO3 (s) is 2.58 x 10-9.1. A sample of an infusion was diluted 10 ml to 250 ml and then 10 ml to 200 ml. It was then analysed and was found to contain sodium at 0.789 mg/100 ml. Calculate the concentration of sodium in the original sample in %w/v. The sample was composed of a mixture of sodium lactate and sodium carbonate in equimolar amounts. Calculate the amount of sodium lactate and sodium carbonate in mg/10 ml of the sample (Na = 23, lactate = 89, carbonate = 60) 2. 0.641 g of a semi-synthetic alkaloid was dissolved in 25 ml of 1% w/v acetic acid and was analysed directly by HPLC. The solution was found to contain 1.42 mg/100 ml of an impurity. What is the level of impurity in % w/w and ppm? 3. Calculate the pH of a buffer system made by dissolving 1.2 g of acetic acid and 0.82 g of sodium acetate in 500 ml of distilled water (pKa of acetic acid = 4.7) 4. Convert the following concentrations into the required expression. Concentration given Expression required 0.5% NaCl molarity 1 mM of KBr…
- 4. determine the amount in mg of the amount of Ag present from ICP mass digested: 1.0821g/L dilution of 10ml stock solution to 100ml volumetric flask X=0.98 (intensity)Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.0700 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