Can someone please walk me through how to do the following problem? Thank you! A typical aspirin tablet contains 324 mg of aspirin (C9O4H8), a monoprotic acid with Ka=2.8 x 10^-4. A monoprotic acid donates a single proton. If you dissolve two aspirin tablets in a 300 ml glass of water, what is the pH of the solution?
How many milliliters of 3.00 M hydrochloric acid would be needed to react completely with a milk of magnesia tablet that contains 310 mg of Mg(OH)2? The neutralization reaction produces magnesium chloride, MgCl2, and water.
Concetration, molarity, mole, volume, limiting reagent, % yield, theoretical yield and actual yield.
Several years ago people who were taking supplements of tryptophan (an essential amino acid that we must take in our food for normal growth and maintenance of a healthy body; without it we could not live) started becoming very ill. Some individuals suggested that tryptophan was what was causing the disease. For most amino acid
1 How many grams of oxygen are required to fill a 4.5 x 103 liter hyperbaric chamber at a pressure of 225 cm Hg and 62 F? If the same quantity of oxygen, was pumped back into a gas cylinder at a pressure of 200 atm and at 75 F, what would the volume be? 2 Any number of green plants can photosynthesize glucose (C6H12O
Predict whether aqueous solutions of each of the following salts are acidic, neutral, or basic. Sodium hydrogen carbonate In class we just learned to look on the table and see if one was a weak acid or strong base, then decide what the solution would be. However, I can't find some of them on the table so then I believe
I just need some help to get started on designing an experiment for a quantitative colorimetric iron assay. We're allowed to use the following items: deionized water 0.02 M feCl3 1,10-phenanthroline ferrozine filter paper test tubes and test tube racks volumetric flasks HCl NaOH digested soil samples undigested s
A titration was conducted to determine the percent of acetic acid within vinegar. The reaction of this titration is HC(2)H(3)O(2) --->NaC(2)H(3)O(2) +H(2)O (water) Given Concentration of NaOH 0.2959 M. Final Buret Reading:26.72 mL Initial buret reading :0.02 mL Volume of NaOH added: 2
What gas is producedd when you add baking soda to soft drinks like: 7Up, Sprite, Orange, Dr. Pepper and Coke? Why does Dr. Pepper produce the most gas? Why does 7Up produce the least gas?
1. What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? (Ksp PbCl2 = 1.6 x 10-5) a. 7.1 x 10-4 b. 1.1 x 10-4 c. 2.0 x 10-3 d. 1.8 x 10-4 e. 1.6 x 10-5 2. In which aqueous system is PbI2 least soluble? a. H2
1. Given the following table of Ksp values, determine which compound listed has the smallest solubility. compound Ksp CdCO3 5.2 x 10-12 Cd(OH)2 2.5 x 10-14 AgI 8.3 x 10-17
1) This is the scenario: there are six prepared solutions, but the labels are not on the bottles. What are the the solutions in the bottle. The six possible solutions are silver nitrate, barium chloride, copper (II) nitrate, copper(II) sulfate, sodium carbonate, and hydrochloric acid. The results were found by mixing the each so
See the attached file. 1. A sample of concetrated nitric acid has density of 1.41g/ml and contains 70% HNO3, by mass. a. What mass of HNO3 is present per litre of solution?(in g/l) b. What is the molarity of the solution? 2. Calculate each of the following quantities. a. molarity of a solution prepared by diluting 3
What is the name of the salt formed by the complete neutralization of sulfuric acid with lithium hydroxide? Choices: 1. hydrogen sulfite 2. lithium sulfate 3. lithium hydride 4. lithium sulfide
What is the pH of a .0078M solution of KOH? Choices: 1. 2.2 2. -2.2 3. -11.9 4. 11.9
What is pH of a .0045M HCl solution. Choices: 1.2.3 2.-2.3 3.11.6 4.-11.6
Boric acid, H3BO3, is found in some laundry detergents, antimicrobials, and pesticides. With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work) 1. Write the equation: 2. What is the pH of the solution before titration begin
Which ion(s) is/are spectator ions in the formation of a precipitate of AgBr via combining aqueous solutions of CoBr2 and AgNO3? a. Co2+ and Ag+ b. Co2+ and NO3- c. NO3- and Br- d. NO3- e. Br- Which of the following is an exchange reaction? a. 2SO(g) + O2(g) ---> 2SO2(g) b. CaCO3(s) ---> CaO(s) + CO2(g) c. F
Calculate the pH upon diluting 2ml of 2 N HCL to a final volume of 100 ml? Calcuate the pH upon addition of 0.0075 mole of solid NaOH to 100 ml of a 0.1 M solution of acetic acid (pKa=4.7)? If equal molar amounts of Na2HPO4 and NaJpo4 are mixed in water, calcuate the resulting pH. The pKas of phosphoric acid are 2.1, 7.2,
A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?
Which of the following cannot act as a Lewis base? A. Cl- B. NH3 C. BF3 D. H2O
Please can you help me, I need to find balanced chemical equations for: a) The reaction of calcium phosphide and water to produce phosphine and calcium hydroxide; b) The oxide formed when phosphorus burns in air, dissolves in water to give a solution of phosphoric acid (H3PO4).
I have a selection of apparatus and materials that I could use to prepare a gas jar of dry phosphine. I have the following pieces of apparatus to use:- Wash bottle Polythene connectors Dropping funnel with rubber stopper Bent glass tube Filter funnel with paper U-tube Porcelain boat Gas jar Round bottomed flask w
Sodium bicarbonate was added to an unlimited amount of sulfuric acid undergoing a reaction to produce sodium sulfate plus carbonic acid (which turned in to water vapor and carbon dioxide upon heating). Please provide a balanced equation for this reaction.
Observations: 1) A reacts spontaneously with 1mol/L BNO3, 1mol/L D(NO3)2 and dilute sulfuric acid.A does not react with 1mol/L C(NO3)2. 2) B does not react with any of the 1mol/L solutions above or the dilute sulfuric acid. 3) C reacts spontaneously with dilute sulfuric acid and with 1mol/L solutions of all the other metallic
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 + 2.5E10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHa? What is pKa of the acid component? I don't understand this problem at all! I know that a diprotic substance has something i
I am really having problems with this problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer. The first part was fair enough, I got 9.35 pH, which is correct. The set up of the second part is tripping me up, I ca
Question 31 What is the molarity of a solution in which 26.0 grams of BaCl2 (molar mass = 208.2 g/mol) are dissolved in enough water to make 450.0 mL of solution? 0.278 M 0.617 M 1.00 M 3.41 M Question 32 Which element has the following electron configuration? 1s22s22p63s2 Na Mg
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 = 2.5E-6. In order to make up a buffer solution of pH 5.8, which combination would you choose, NaHA/H2A or Na2A/NaHA? I know the solution is Na2A/NaHA, but I am not sure why. What is the pKa of the acid component?
How much NaOH is needed to prepare 576 mL of solution with a pH 10? Is it possible to calculate concentration of a solution, OH- concentration, and H+ concentration from just a pH given (no specific base or acid)? Is the concentration of a solution the same as the concentration of [OH-] or [H+]?