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- Drug A dissociates into four ions to the extent of 70%. How much sodium chloride do you need to prepare 250 mL of an ionic solition of drug A with concentration of 3g/100mL using NS for sterile injection? MW of Drug A= 892.54 (assume final volume will be qs with sterile water for injection) a. 155.9 ml NaCl b. 62.37 mL NaCl c. 146.6 mL NaCl d. 218.33 mL NaClRun 1 Run 2 Molarity of KMnO4 solution (M) from bottle 0.00101 0.00101 Initial reading of buret KMnO4 (mL) 0.62 11.35 Final reading of buret KMnO4 (mL) 11.33 21.70 Run 1 Run 2 Volume of KMnO4 solution (mL) Moles of MnO4- used for titration (mol) Moles of C2O42- in 100.0 mL of solution (mol) Molarity of C2O42- (M) Molarity of Cd2+ (M) Ksp of CdC2O4 Average Ksp of CdC2O4 Calculations: Moles of MnO4- used for titration of saturated solution CdC2O4 Moles of C2O42- in 100.0 mL of saturated solution of CdC2O4 Molarity of C2O42- in saturated solution of CdC2O4 Molarity of Cd2+ in saturated solution of CdC2O4 Solubility product, Ksp, of CdC2O4Please help with calulation of theoretical yield of the following: Na2CO3 + Ca(NO3)2.4H2O ---> CaCo3 + 2NaNo3 + 4H2O 2.03g Na2CO3 2.06g Ca(NO3)2.4H2O
- If this lab’s procedure were carried out using 28.06 mL each of 0.385 M K2CrO4 and 0.161 M Pb(NO3)2. How many mmol of K2CrO4 were present in the reagent solutionA 25.00 cm3 solution containing Ni2+ was treated with an excess of an ammoniacal solution of dimethylglyoxime (dmgH2) and 0.7223 g of Ni(dmgH)2 was precipitated. What is the molarity of Ni2+ in the solution in mol dm–3? [Mr / g mol–1: Ni(dmgH)2 = 288.9149] a. 1.000 × 10–3 mol dm–3 b. 1.00 × 10–1 mol dm–3 c. 1.0 × 10–1 mol dm–3 d. 1.000 × 10–1 mol dm–3 e. 1.0 × 10–3 mol dm–3Sodium carbonate is a reagent that may be used to standardizeacids in the same way. In such standardization it was found that a 0.432-g sample ofsodium carbonate required 22.3 mL of a sulfuric acid solution to reach the end point forthe reaction.Na2CO3(aq) + H2SO4(aq) -----> H2O(l) + CO2(g) + Na2SO4(aq)What is the molarity of the H2SO4?
- Mass of crude Acetanilide = 0.508 Mass of filter paper = 0.800g Filter paper + pure Acetanilide = 1.153g Mass of pure Acetanilide = ? % recovery = ? Mpt of recrystallized Acetanilide =112 C – 114 C Mpt of crude Acetanilide = 97 C – 110 CPrepare 0.1 M solutions of NaOH and 0.1 M ethyl acetate using high-purity distilled water. So, weight desired amount of NaOH and ethyl acetate and dissolved in dH2O to prepare stock solution in equal molarity. Mw (NaOH) = 40.0 g/mol , Mw (EtOAc)= 88.1 g/mol, Density(EtOAc): 0.898 g/cm3Calculate the mass percent of the ascorbic acid in the same show full solution Situation: The pounded Vitamin C tablet was half into two below are the calculated data in the experiment. Each of the half are transfered in a 250ml erlen meyer flask and added 75ml of deionized water for the vitamin C to dissolve. Then it was prepared for titration where the burette was filled with 0.09794M standardize NaOH solution then a total of with 3 drops 2% phenolphthalein indicator was added to each erlen meyer flask l, swrill it and begin the titration. below are the following data gathered: Vitamins used: Nature Made vitamin C 500mg tablet Trial 1 Mass: 0.3108g of Vitamin C tablet Initial volume: 1.6mL Final volume: 15.4mL Trial 2 Mass: 0.3349g Initial volume: 15.4 mL Final volume: 30.2 mL
- A 19.51 ݃ sample of impure methylamine, which contains 72.58% (by mass) of CH3NH2 , isreacted with 30.81 ݃ of pure oxygen gas:4CHଷNHଶ(g) + 9Oଶ(g) ⟶ 4COଶ(g) + 10HଶO(ℓ) + 2Nଶ(g) In another experiment, this impure methylamine was used as follows: An unknown mass of the impure compound is dissolved in enough water to make 500.0 ݉ܮof solution. 20 ݉ܮ of this solution was transferred by pipette to a clean 250 mL volumetric flask andmade up to the mark. The molarity of the CH3NH2 in the final solution was determined to be 0.103 M.Determine the mass of CH3NH2 present in the original amount of impure compound used tomake this solution.Recall that the formula for ΔHrxn = [(-Ccal)(moles of limiting reactant)/(ΔT)]If the actual concentration of the sodium hydroxide used in the calibration part of the experiment was lower than the stated value, will the value of Ccal increase, decrease, or remain the same? Please explain. How about if the actual concentration of the sodium hydroxide used in the calibration part of the experiment was lower than the stated value. However, the NaOH solution used in the determination of ΔHrxn was of the correct concentration. Will the magnitue of ΔHrxn increase, decrease, or remain the same? Please explain.A 0.53 g sample containing KBr (MW=119) is dissolved in 50 mL of distilled water. Titrating with 0.04614 N AgNO3 requires 28.5 mL to reach the endpoint. Calculate the %w/w KBr in the sample. (Round-off your answer to 2-decimal places) Answer = ____%