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Can I have help with these questions? I would like to practice the solutions to these problem. 1. A sample of water has 24 grains per gallons of hardness as calcium carbonate. What is the hardness in terms of mg/L. 2. How many kg of chlorine gas should be dissolved in 5 million liters of waters to result in a concentratio
5) Using the following pKb (pKb = 4.11) of an unknown base, calculate the Ka of the corresponding conjugate acid and use the Ka value to identify the unknown base. Be careful to show all the steps used to convert pKb to Ka. (See attachment for data) 6) Potassium hydrogen phthalate (KHP, K+OOC-C6H4-COOH) is a carboxylic acid
By using samples of the same cerium solution throughout each trail and precise volumetric pipettes, accuracy, along with precision, the potential change of the reaction and the determination of the molar concentration of iron (II) ions in a sample of unknown concentrations were determined by potentiometric titration of the react
Titration of Strong and Weak Acids. Determination and assessment of equivalence points. Calculation of molarity. Estimation of acid/base equilibrium constant, pKa
Procedure 1 Add 25 mL HCl (of unknown concentration) to the flask. Add 2 drops of phenolphthalein to the flask. Fill a burette with 50 mL of 1M NaOH solution. Record this initial volume (50mL). Record the pH of the solution in the flask. (0.22). Continue to add NaOH in 1 mL increments. Record the pH for each milliliter added.
1. Write the complete ionic and net ionic equations for the reaction between AgNO3 and K2CrO4. Molecular equation: 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq) 2. Write the complete ionic and net ionic equations for the reaction between AgNO3 and NaCl. Molecular equation. AgNO (aq)+NaCl(aq)---à AgCl(s)+NaNO (aq)
1) Plot the pH titration of tyrosine, whose structure is shown attached at pH = 7.0. Show: a) The pH value at each equivalence points and each 1/2 equivalence point b) The charge at each equivalence and 1/2 equivalence point c) The isoelectric point of the amino acid and give its value d) The approximate shape of the titrat
A 30 mL sample of 0.35 M of lactic acid is titrated with a 0.25 M NaOH solution. Calculate the pH before NaOH is added. After 20 mL of NaOH is added. After 42 mL. After 45 mL. After 60 mL. After 80 mL. Graph the titration curve.
C6H5COOH ( benzoic acid ) = C6H5COO- (aq) + H+ (aq) Ka = 6.46 x 10^-5 Benzoic acid dissociates in water as shown in the equation above. A 25.0 ml sample of an aqueous solution of pure benzoic acid is titrated using standardized 0.150 M NaOH A) After addition of 15.0ml of the 0.150 M NaOH , the pH of the resulting solution is
1. Vitamin C is considered to be unstable during cooking. What kind of chemical reaction do you expect vitamin C to undergo in solution (hydrolysis, oxidation, reduction?) 2. If 12.5 ml of iodine solution is needed to titrate 10.0 ml of 1.0 mg/ml ascorbic acid standard solution and 5.0 ml of iodine solution is needed to titr
A solution is made by mixing 13.0g of NaOH and 77.0 mL of 0.160 M HNO3 . Calculate the concentration of OH- ion remaining in solution. Calculate the concentration of Na+ ion remaining in solution. Calculate the concentration of NO3- ion remaining in solution.
First I dissolved a 250 mg tablet of vitamin c in 50 mL distilled water. Then, I prepared a buret with 0.002034M KIO3 solution Next, I pipetted 5.00 mL of the vitamin c solution into a flask and added 5 mL of 0.6M KI solution, 5 mL of 1M HCl, 1 mL startch indicator solution. The endpoint was reached after 11.27 mL of KI
Titration Acid/Base Exactly 100ml of 0.12 Molar nitrous acid (HNO2) are titrated with a 0.12 molar NaOH solution. Calculate the pH for--- A. the initial solution B. the point after 80ml of the base has been added C. the equivalence point D. after 105ml of base has been added
Calculate Titration. See attached file for full problem description. 19. Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 25.0 mL of 0.200 M HA with 0.100 M NaOH. Ka = 2.0 * 10^-5. 20. Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 50.0 mL of 0.100 M N
How many millimeters of 0.500 M NaOH should be added to 10.0 g of tris hydrochloride to give a pH of 7.60 in a final volume of 0.250 mL? Useful information: Tris hyrochloride fw = 157.596 g/ml The Kb for tris is 1.2 x 10^-6 You can represent tris hydrochloride as BH+ and its conjugate base, tris, as B.
1. (A) Assume you have a solution containing 0.1 mol of Ala adjusted to pH = 0.5 with HCl. You begin adding 1.0 M NaOH. Plot (do not sketch) the resulting titration curve (pH vs. moles NaOH added) showing all inflection points. Show your calculations and be sure to state your assumptions. (B) Plot a similar titration curve f
I have a big Chemistry test Friday, and I have to learn how to find the average molarity of NaOH (0.1 M) from three trial titration experiments I did in lab. Titration #1 Volume of NaOH used =3.9 ml Titration #2 Volume of NaOH used = 3.9 ml Titration #3 Volume of NaOH used = 4.0 ml.........AVERAGE MOLARITY OF NaOH___
A titration with potassium permanganate is used for the oxalic acid 5H2C2O4+2Mn)4- +6H+ ------->10CO2+2Mn2+8H2O calculate the molarity of an oxalic acid solution requiring 23.2 ml of 0.127 M permanganate for a 25.O ml portion of solution Is this set up as a ratio? If so, How do I set it up?
A .823 g sample of an ore of iron is dissolved in acid and converted to Fe2> The sample is oxidized by 38.50 ml of 0.161 M ceric sulfate, Ce(SO4)2 soltion, The cerium 4 ion Ce4+ is reduced to Ce3+ Ion. What is the percent iron in the ore?
I have several problems dealing with titration one of them deals with iron in a 5.675 g sample containing Fe2O3 reduced to Fe+2. TheF+2 is titrated with 12.42 ml of 0.1467 M K2Cr2O7 in acid solution. How do I go about finding the mass of iron and the percent of iron in the sample.
I am having trouble with this one problem. It is a couple of steps but I am very confused. The problem states that there is 25 mL of a propionic acid where the concentration is unknown and it was titrated with .104M KOH. I got the Ka=1.34*10^-5 for the propionic acid. It also tells you that the equivalence point was reac
The following attached file are two problems that are not 1:1 stoichiometry titration problems. The first problem is broken down to five parts and it involves a precipitation titration problem. The second involves a back titration.
Please give simple, step by step solutions. Thanks! 1) Write the molecular, ionic, and the net ionic equations for the reaction between aqueous potassium carbonate and aqueous lead(II) chloride to form aqueous potassium chloride and a precipitate of lead(II) carbonate. Molecular equation: Ionic equation: Net ionic e
Draw the titration curve for the titration of a 0.05M solution of acetic acid with 0.1M sodium hydroxide. I can find the initial pH of the solution, but I am not given any initial volumes so can you point me in the right direction of how to solve this problem? If I don't need volumes can you give me a hint as to how this pr
What's the pH at the first equivalence point of 0.100M of malonic acid of 25mL with 0.140M of NaOH? What's the pH after 25mL of NaOH were added?
If 25.00 mL of 1.000M HNO^3 is titrated to a neutral endpoint with 36.97 mL of NaOH solution, what is the molarity of the NaOH solution?
10.00 mL of HCl is titrated to a neutral endpoint with 35.78 mL of 0.200M NaOH. What is the molarity and normality of the HCl?
How many milliters of 3.50M HCl is needed to react with 400.0 mL of 2.1M CaSO4 in the following reaction? HCl + CaSO4 yields CaCl2 + H2SO4
A sample of 0.0054 mol propanoic acid was dissolved in water to give 50ml solution. This solution is titrated with 0.150 M of NaOH. Draw the expected titration curve labeling the equivalence point (including the volume of NaOH added and the pH) and show the pKa point (labeling the pH value and volume of NaOH added)
Outline a titration procedure for determining the exact concentration of the aqueous nitric acid. Assume that aqueous sodium carbonate of concentration 0.500 mol dm3 is available.