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Acids and Bases

3 Chemistry Multiple Choice Questions

1. The half reaction of NpO2+ to Np+4 is a. an acid-base reaction b. a redox reaction c. reduction d. oxidation 2. The standard hydrogen electrode has a half-cell potential of 0.00v. This is due to a. arbitrary convention b. hydrogen gas being insoluble in water c. coincidence d.

Chemical Reaction Problems

1. The following is best described by which type of reaction? CaCO3 --> CaO + CO2 A. decompostion B. acid-base neutralization C. single displacement D. redox E. double-displacement (metathetical) 2. The following best describes which type of reation? 2Ca + O2 --> 2CaO a. decomposition b. acid-base neutraliz

Determine solubility of boric acid (H3BO3) at various pH's

This problem indicates that 1 gram of hydrated boric acid (H3BO3) is added to 1 liter of water at pH 7.0 and at standard temperature. The solubility is stated in the problem as 5.7 grams per 100 ml of solution. A pKa is also given as 9.24. 1) What does the pKa value mean? 2) How would I determine the amount of boric acid

What type of reaction does this describe?

What type of reaction does this describe? metal + H2O --> metal oxide + H2 a. decomposition b. acid-base neutralization c. single displacement d. redox e. double-displacement (metathetical)

Solubility of reaction

The Ksp for Fe(OH)2 is 1.8 x 10-11. Will a precipitate form if an 0.4M solution of FeCl2, has its pH raised to 8.3? What is the solubility of Mg+2 in 0.03M HF? Ka for hydrofluoric acid is 6.6 x 10-4. The Ksp for magnesium fluoride is 3.7 x 10-8 Also: Complete the following reactions: a. H2PO4^- +H^+ ->

Vitamin C Content of Juices

Assignment 1 of Procedure 1 1. Calculate the molarity of the freshly-prepared ascorbic acid standard (known strength) solution: (a) Mass of ascorbic acid used:0.05g (b) Moles of ascorbic acid (MW=176.1 g/mol):not sure 0.000284 (c) Total volume of standard solution prepared (mL):100.01mL (d) Asc

Equilibrium and Acid - Base Reactions

1. The Ka for HF is 6.6 x 10^-4. What percentage of the HF is ionized if 5 grams are dissolved in 1 liter of water? 2, Assume an indicator, HA, has a Ka od exactly 10^-7. This means that at pH = 7 there are equal numbers of molecules of both colors. What is the ration of colors at pH values of 7.2 and 8.0?

Equilibrium and Acid-Base Reactions

1. The hydration reaction , Na2HPO4 + 2H2O -> Na2HPO4 x 2H2O has a Kp = 6000 at 300K If excess dry, anhydrous Na2HPO4 is added to a 3L container holding 25mmHg of water vapor, what will be the pressure of water after it equilibrates with the sodium phosphate? 2. What is the pH if 2g of NaC2H3O2 and 1g of HC2H3O2 are mixed


My text book lists "ordinary vinegar" as having a pH of 2.4. Using the data from the attached problem find the concentration of acetic acid in vinegar.


1. Which of the following could NOT be a Bronsted-Lowry base? a. HCO3- b. F- c. SO3-2 d. NH4+ 2. What is the pH of a 0.1M HCl solution? a. 0.1 b. 0 c. 1 d. 10 3. Which is the stronger (more highly ionized) acid? a. HF b. HCl c. HBr d. HI 4. Which of

PH of a solution of a weak base

The pH of a 0.12 M solution of a weak base is 10.30. What is the value of pKb for this weak base? a.) 3.70 b.) 6.48 c.) 10.30 d.) 5.44 e.) 4.49

The value of Kb

The value of Kb for methylamine, (CH3)2NH, is 7.4 x 10 ^ -4. What is the pH of a solution containing 0.32 M dimethyl ammonium ion, (CH3)2NH2 + ?

Glucose Synthesis

Glucose is soluble in benzene. If α-D-glucose is dissolved in benzene, essentially no β-D-glucose is formed. However, if small amounts of phenol and pyridine are added, then the equillibrium amount of β-D-glucose is formed but slowly. If, to a solution of α-D-glucose in benzene, a small amount of 2-hydrox

Hydrogen Ion Concentration

How do you find hydrogen ion concentration, and which of the following have the highest concentration? 55.6M H2O 0.25 M HCl 1.0 M CH4 1.2 M NaOh 0.20 M NaH

Acid-Base Equilibria

1. Write formulas for the conjugate bases for each of these acids: a) HCl b) CH4 c) HSO3- d) H2SO4 e) NH3 2. In the following reactions, identify the Lewis acid and the Lewis base: a) Fe3+ + 6H2O ←→ Fe(H2O)36+ b) BF3 + NH3 ←→ F3BNH3 c) BF3 + F- ←→ BF4-

Chemistry Element Questions

1. What is the volume of 1.20 x 1022 molecules of nitric oxide gas, NO, at STP? 2. What is the mass of sodium phosphate (163.94 g/mol) that yields 1.00 g of calcium phosphate (310.18 g/mol) precipitate? __CaCl2(s) + __Na3PO4(aq) → __Ca3(PO4)2(s) + __NaCl(aq) 3. How many moles of calcium metal react to yield 0.50


1.) Calculate the four values of pH, pOH, [H+], and [OH-] for a 0.100 M of HCl. 2.) Calculate the four values of pH, pOH, [H+], and [OH-] for a 0.00250 M NaOH solution. 3.) Calculate the four values of pH, pOH, [H+], and [OH-] fo a 0.00150 solution of nitric acid (HNO3). 4.) The Ka of HCl is known to be about 10^7. What is th

Mole, Mass, Enthalpy, and Energy Change Problems

See attached file for full problem description. 1. Which is not a solution? brass, fog, hydrochloric acid, or wine 2. How Many Moles of CuO can be produced from 0.0450 mol if Cu2O in the following reaction? 2 Cu2O(s) + O2(g) -> 4 CuO(s). 3. Methane and Oxygen react to form carbon dioxide and water. What mass of wa

Sulfric acid H2SO4

A 0.21g sample of sulfuric acid is dissolved completely in water to make 0.25 litre of final solution. Calculate the hydrogen ion concentration in mol 1 - 1 in this solution. In scientific notation and significant figures.

Calculating mass of sulfuric acid to affect pH change?

I have a 2 part question concerning the use of H2SO4 to adjust the pH of a solution: 1. How many grams per liter of H2SO4 is required to adjust the pH of a solution from 3.8 to 2.8 assuming the sulfuric acid fully ionizes? 2. If in reality however, the actual sulfuric acid ionization/dissociation is a 2 step process and no

Formation of Aluminum Hydroxide from Aluminum Sulfate and Water

Assume we have a 1000L tank of water and very dilute weak acids. To this tank we add and dissolve 260 grams AL2(SO4)3 (solid granules) --- the resultant pH is 4. The intention is to form AL(OH)3 solids/particles in this reaction. Question 1: How much Al(OH)3 will be formed in this reaction at pH=4.0 Question 2: If the pH w

Calculate amount of NaOH to raise an acetic acid and water pH

Please walk me through the calculation of determining how much NaOH is needed to raise a 1 liter solution of acetic acid and water with a pH of 4.5 to a final pH of 6.0 ---- this would be at 25 degrees C? What happens in this system if temperature is 55 degrees C?

Basic Techniques in Cell Biology and Biochemistry

The only problems that need to be done are numbers (3) and (4) on the second scanned document and the question below . Numbers (1), (2), (5) are finished problems that do not need to be done so problems (3) and (4) should be done using the same format (do Calculations and preparation)as those. Also please answer this ques

pH and Molarity

Please help with the following problems. a.) Giving the reason for your answer, which would you expect to have the higher value of pH, a 1.0M solution of the strong acid, HCl or a 1.0M solution of the weak acid, acetic acid, CH3COOH? b.) Why is it that we can say that ozone in the stratosphere is beneficial to

Stoichiometry Problems, Limiting Reagent, Acid/Base, Balancing Chemical Equations

1. A solution is prepared by dissolving 10.8g ammonium sulfate in enough water to make 100.0mL of stock solution. A 10.00mL sample of this stock solution is added to 50.00mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution. 2. One of the most commonly used white pigments in paint

Quantative Analysis of Acid in Vinegar

Acid content of vinegar Flask 1 Flask 2 Inital volume of NaOH in burette 0 17.5 Final volume of NaOH in burette 17.5 35.3 Volume of NaOH used for titration


PH OF A BASIC SOLUTION. PH is defined as the negative logarithm of Hydrogen ion concentration. Strength of a base is expressed as the concentration of OH- ions. Therefore PH of a basic solution can be calculated using the relation Kw=[H+][OH-]=1x10-14 at 25degree celcius PH=-log[H+] Problem: Calculate the PH of a s