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Acids and Bases

pH of a Solution Given its Composition

Acetic acid (CH3COOH) is a weak acid with the following ionization reaction: CH3COOH + H2O Û H3O+ + CH3COO- Ka = 1.8 x 10-5 What is the pH of a solution that is 0.5M in acetic acid and 2.5M in sodium acetate, CH3COONa?

Volume of Sulfuric Acid

What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.1 M sulfuric acid? a. 9.4 mL solution b. 9.4 L solution c. 16 mL solution d. 16 L solution

Benzoic acid with hydroxide ion - extraction with sodium hydroxide

Show an equation for the reaction of benzoic acid with hydroxide ion? If you were performing an experiment with a Grignard reagent phenylmagnesium bromide with dry ice (carbon dioxide) in ether to create benzoic acid, why would it be necessary to extract the ether layer with sodium hydroxide?

Solving for the products of reactions

(See attached file for full problem description) --- 1. Fe²+ and Sb³- 2. Mg²+ and As³- 3. Al³+ and O²- 4. Co³+ and I- 5. Sr² + and P³- 6. Ca²+ and C4+ 7. Fe³+ and As³- 8. Na + and S² ˉ Write the name or formula for these compounds: 1. tin (II) acetate 2. bromous acid 3. copper(II) permanganate

Chemistry Ka and Kb problems

1. Butyric acid is responsible for the odor in rancid butter. It has one weakly acidic proton. A solution of .25 M butyric acid has a pH of 2.71. Determine the Ka of the acid. 2. Ka for HCN is 4.0 x 10^10. Calculate Kb for CN. 3. For the equilibrium, CH3OH (g) <-- --> CO (g) + 2 H2, Kc is 6.9 x 10-2. At equilibriu

Mechanisms for three reactions

Sn + 2I2 ---> SnI4 (Ac2O,AcOH,reflux on arrow) SnI4 + 2PPh3 ---->(PPh3)2SnI4 (CHCl3 on arrow) SnI4 + (Me2SO)2 ----> SnI4(Me2SO)2 (CH2Cl2 on arrow) Give mechanisms for these reactions if there is any.

Solubility Problems with Ksp

Q#1 (Common ion problem) What is the solubility,in mg/mL of BaF2 in a)Pure Water b)in a solution containing 5.0mg/mL of KF Ksp of BaF2=1.0*10^-6 Q#2 Effect of pH on solubility a)Calculate the solubility of a saturated solution og Mg(OH)2 on pure water.(My answer is 1.65096*10^-4M b)Calculate the solubility of the sa

Applications of Aqueous Equilibria

50.00 mL of a 1.00 M solution of the diprotic acid H2A (Ka1= 1.0 * 10^-6 and Ka2 = 1.0 * 10^-10) is being titrated with 2.00 M NaOH . How many mL of 2.00 M NaOH must be added to reach a pH of 10?

Hess' Law of Additive Equations for Reactions

Using Hess' Law of additive equations, rearrange and/or multiply the following reactions in order to find the enthalpy for the radical reaction between hydrochloric acid and isopropyl alcohol (CH3CHOHCH3) to form water and isopropyl chloride. The dots you see indicate a radical, which is much different than an ion or an element

Solubility and Titration

(See attached file for full problem description) --- 1. Tooth enamel consists of hydroxyapatite, Ca5(PO4)3OH (Ksp = 6.8x10-37). Fluoride ion added to drinking water reacts with Ca5(PO4)3OH to form the more tooth decay-resistant fluorapatite, Ca5(PO4)3F (Ksp =1.0x10-60). Fluoridated water has dramatically decreased cavities

Lab experiment titrating hydrochloric and acetic acids with NaOH

I would like to see the details of the calculations. For my lab experiment I have the following data: Titration 1: 25.00mL of unknown concentration HCl 2 drops of phenolpthalein to show end-point 1.0M NaOH What is the molarity of the HCl? What is the Ka of the HCl? What is the equivalence point? What is the half-equival

pH Effect on Solubility & Expressions

3. Why does pH affect the solubility of CaF2 but not CaCl2? 4. Write the correct expression for Ksp for Al(OH) 3. (See attached file for full formatting)

pH After Titrations - Ionic Equilibria

1. Calculate the pH after 25.0 mL of .20 M HF (Ka=6.8 10-4) are titrated with 15.0 mL of .10 M NaOH? 2. Calculate the pH after 25.0 mL of 2.0 M HF is titrated with 50.0 mL of 1.0 M NaOH?

Titration Calculations

Note: You may assume that the densities of all solutions are 1.00 g/mL unless stated otherwise 1. A 10.00-mL sample of a solution containing the weak acid, formic acid, was placed in a 25-mL volumetric flask and diluted to the mark with water. A 10.00-mL sample of the diluted formic acid solution was then titrated with 0.13

Using Titration Techniques

1. If a strong acid and weak acid have the same concentration of acid, explain why they will have a different pH. 2. Explain why it is important to prime the pipette. 3. When using the titration technique explain why the beakers that contain the acid solutions must be dry before the acid is added, but the volumetric flask

Determining pH of weak acid

(See attached file for full problem description) 3. Calculate the pH of 0.25 M HOAc. 4. Calculate Kb for OAc- .

Solubility Characteristics of Carboxylic Acids

1) If you took a pea-sized amount of salicylic acid and added 2 mL of demineralized water, what would the solubility of salicylic acid in the water be? 2) If you then added 5 drops of 6 M NaOH to the mixture, what would the solubility of salicylic acid in a base be? 3) I know the result of this is sodium salicylate, whi

Weak Base Reaction Calculations

Can someone please walk me through how to do the following problem: If a solution is made by mixing 20.0 ml 0.4 M NaCH3COO with 30 ml 0.4 M CH3COOH, calculate the pH. For acetic acid, ka = 1.76 x 10^-5.

Acid dissociation reaction.

Can someone please walk me through how to do the following problem? Thank you! Consider the following equation at equilibrium. CH3COOH <---> CH3COO- (aq) + H+ (aq) If NaCH3COO is added to the solution, indicate if the following quantities will increase, decrease, or stay the same -- and explain why for each. [H+] [O

Calculating Ka for Formic Acid

Can someone please walk me through how to do the following problem? Thank you! For a 0.13 M solution of formic acid, HCOOH, the pH = 2.40. Calculate Ka for formic acid. HCOOH <---> HCOO- (aq) + H+ (aq)

PH, Ka

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?

Calculating pH Levels

Can someone please explain to me the following question? "Calculate the pH of a 1.0 M CH3COOH solution." My answer: pH = -log[H+] = -log[1.0] = 0 But how can that be right? Since CH3COOH is a weak acid, how can it have a pH of zero? Did I do something wrong?

Mol/Mol Calculation: Detailed 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.

To calculate percentage yield

For the reaction SO3 + H2O yields H2SO4, calculate the percent yield if 500.g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid? 82.7%, 88.3%, 91.2%, 93.9%