Problem Solving Read CAREFULL each statement and report your answers: - Volume, and Percentage strength should be rounded off to two decimal places, - Weight, Normality should be rounded off to four decimal places 107. The USP requires that hydrochloric acid contain not less than 35 and not more than 38 % w/w HCI. You are about to assay a sample of HCI (MW=36.46g/mol; sp gr 1.18) following the procedure below: 1) Accurately weigh 4.0520 in glass-stoppered flask while containing 45mL of water 2) Add methyl red ts 3) Titrate with 0.9035N sodium hydroxide 4) After titration, it was found out that 44.15mL of volumetric solution used to bring the reaction to end point and 4.15mL volumetric solution used in blank titration a) What type of titration occur on the titration? b) What is the name of the salt form from the neutralization reaction c) Calculate the percentage composition of HCI in % w/w d) Does the sample conforms to the official requirements?

Problem Solving Read CAREFULL each statement and report your answers: - Volume, and Percentage strength should be rounded off to two decimal places, - Weight, Normality should be rounded off to four decimal places 107. The USP requires that hydrochloric acid contain not less than 35 and not more than 38 % w/w HCI. You are about to assay a sample of HCI (MW=36.46g/mol; sp gr 1.18) following the procedure below: 1) Accurately weigh 4.0520 in glass-stoppered flask while containing 45mL of water 2) Add methyl red ts 3) Titrate with 0.9035N sodium hydroxide 4) After titration, it was found out that 44.15mL of volumetric solution used to bring the reaction to end point and 4.15mL volumetric solution used in blank titration a) What type of titration occur on the titration? b) What is the name of the salt form from the neutralization reaction c) Calculate the percentage composition of HCI in % w/w d) Does the sample conforms to the official requirements?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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RESET 9) Draw a picture of what happens to the formula units in the following aqueous solutions. Do not draw the water molecules; just the particles present after dissolving the compounds. Assume you have 4 acid molecules dissolved in each beaker. See examples on page 499-500 of text. HC;H3O2 (aq) HCl (aq) ||| |||| Cancel Done 中。
What is the concentration of H3O+ and OH- in 0.59 HCl. (Kw = 1.0 * 10-14)
Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sampleand record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter . Calculate the Ksp for each trial and theaverage Ksp and record these values inData Table 1. Ksp = [Ca2+][OH-]2 Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl Volume in Syringe 1.0ml…
How many milliliters of water have to be added to 122.5 mL of 0.50 M HCl to reduce the concentration to 0.10 M HCI? Vwater mL %3D eTextbook and Media Hint Save for Later Attempts: 3 of 15 used Submit Ans ост 14 tv MacBook Air 80 888 DD F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 @ 23 2$ 4 7 OC
A solution is prepared by dissolving 0.13 mol of formic acid and 0.13 mol of ammonium chloride in enough water to make 1.0 L of solution. (K₂ (HCOOH) = 1.8 × 10−4, Kb (NH3) = 1.76 × 10-5) Part A Find the concentration of ammonia in the solution. Express your answer in moles per litre to two significant figures. View Available Hint(s) ΨΕ ΑΣΦ [NH3] = 0.13 Submit Previous Answers ? Review | Constants | Periodic Table mol L-1 X Incorrect; Try Again; attempts remaining The entered value is the initial amount of NH4+ in moles in 1.0 L of a solution. Prepare two ICE tables using a balanced equation for the ionization of NH3 and HCOOH. First, calculate the concentration of H3O+ since it influences the dissociation of NH4+.
. Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 2. 0.1M HCl = 0.1 moles HCl / 1 Liter solutionCalculate the moles of OH- in each sampleand record these values in Data Table 2. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 2. Ca(OH)2 Ca2+ + 2OH24. Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.37 25.37 25.37 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.18 28.21 28.28 Mass of Calcium Hydroxide Solution Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl volume in Syringe 1.0ml 1.0ml 1.0ml Final HCl volume in Syringe .54ml .58ml .5ml Volume of HCl Delivered .46ml .42ml…
$ 1 The hydroxide lon concentration of an aqueous solution of 0.589 M hypochlorous acid is [OH-] = R F Submit Answer 888 F4 % 5 T G M. Retry Entire Group 9 more group attempts remaining FS Cengage Learning Cengage Technical Support ^ 6 MacBook Air Y H & 7 U * 8 F8 ( 9 needed for this question. A F9 O ) 0 F10 P 4) F11 Previous Next> Save and 1 11
Question 2 of 12 Submit The concentration of hydroxide ion in an aqueous solution at 25°C is 5.4 x 10-4 M. What is the concentration of the hydronium ion? | M 1 2 3 4 6. C 7 8 +/- x 10 0 Tap here or pull up for additional resources LO
If you needed 200 L of 6M HCl for your pool, what volume of your unknown HCl would you need to add instead( if it's not 6M) SHOW WORK!
1 Settings „l ? 9:57 AM • 97% kzb-vvdv-bir » Grace Dykstra is presenting TAM Mo Fa 2 H the amount of water added was 1000 mL instead. Would t V ז ןיידצל 1oODmL - LoNIcediud Lies solvent) concentrated than the initial KOOL-AID? Examples: Concentration Calculations Part A Determining Concentration from moles and V: (answers: 0.46 mel; 247 mol ; 0.658 ma) 1. Determine the molar concentration when 0.23 mol of sodium sulfate are dissolved in 500ml of water. G: lo00 0.50ol 0.a3 mol 0.50OL 0. a3 mol = 0.4b mol /L mol 0.500 L 1. 2. Determine the concentration when 1.20 moles of sodium hydroxide dissolves into 450 ml of water. 3. Determine the concentration of a Nacl solution if 25.0 g of sodium chloride is dissolved into 650 ml of water. Alyssa Khadija You Grac 22 others
the References to access Important values if needed for this question. What concentration of barlum hydroxide is needed to give an aqueous solution with a pOH of 1.220? Molarity of barlum hydroxide = M Submit Answer 288 R F4 % 5 Show Hint .:: T Retry Entire Group G F5 Cengage Learning Cengage Technical Support ^ 6 9 more group attempts remaining MacBook Air Y H & 881 7 ◄◄ F7 U 8 F8 1 9 F9 O 0 F10 P 4) .. Previous F11 Next 11 Save and Ex 10
Calculate the maximum volume in mL of 0.15 M HCl that each of the following antacid formulations would be expected to neutralize. Assume complete neutralization. (Show work.) a) a tablet containing 250 mg Al(OH)3 and 150 mg Mg(OH)2 b) a tablet containing 850 mg of CaCO3