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Acids and Bases

PH and Indicator Lab Report

PH Indicator Procedure #1 pH Indicators for Acids: 1. Take seven clean test tubes from the Glassware shelf and place them on the workbench. 2. Add 5 mL of 0.1M HCl and 5 mL of water from the Chemicals shelf to the first test tube. 3. Add 9 mL of water to the 6 remaining test tubes. 4. Pour 1 mL of the solution fr

Using Equilibrium with Calcite and CO2.

Please see the attached file for the fully formatted problems. KH = 3.3 x 10-7 Ka1 = 4.5 x 10-7 (carbonic acid) Ka2 = 4.7 x 10-11 (bicarbonate) Ksp = 5 x 10-9 (calcite) Assuming equilibrium between the atmosphere, seawater, and calcite: [H+]3 = KH2Ka12Ka2PCO22 2Ksp [HCO3-] = 2Ksp{H+]2

Antacids : Gram Equivalent of Hydroxide Ion

Problem: Using the equivalent millimoles HCl/mg sample, the stoichiometry of reaction of HCl with NaOH (which I know is 1:1), and the molar mass of the hydroxide ion, report the gram equivalent OH- per gram of ...there is moreshow problem Using the equivalent millimoles HCl/mg sample, the stoichiometry of reaction of HCl with

Lead Solubility

Please provide solution for (a) and (b) with explanation of how it was derived. Early groups used Pb plumbing in their homes more than 2000 years ago. This Pb pipe has since corroded in the soil to form cerrusite (PbCO3) and hydrocerrusite ( Pb3(CO3)2(OH)2 ). Essington et al., 2004. The soil mineralogy of lead at Ho

Inorganic Chemistry - Strong and Weak Acids

Sulfuric acid H2SO4(aq) is described as a strong acid whereas hydrofluoric acid HF(aq) is described as a weak acid. (a) (i) Describe what is meant by the terms strong and weak acid. (Two or three short sentences) (ii) Write fully balanced equations for the equilibrium dissociation of both sulfuric and hydrofluoric acids in

Concentration, titration, pH and pOH of solutions.

Please see the attached file for the fully formatted problems. Problem 10.53 What is the molarity of an HCl solution if 11.0 mL HCl solution is titrated with 21.6 mL of 0.130M NaOH solution? HCl (aq) + NaOH (aq)  NaCl (aq) + H2O (l) Problem 10.85 What are the [H3O+] and [OH-] for a solution with the following

Solutions : Acids, bases, Salts, pH and Concentration

Label each of the following as an acid, base or salt, explaining your answer: a. KOH b. HCl c. Ba(OH)2 d. H3PO4 e. FeSO4 2. Calculate the pH of the following solutions with the given [H+] or [OH-] and indicate whether it is an acid or base: a. [OH-] = 0.01 b. [H+] = 0.001 c. [OH-] = 0.0

buffer solution challenged by HCl

I have four problems that I don't understand how to figure out. I've done problems 16-20 but don't know how to do 21-24. I've attached the whole page from the exam for the information it provides. I've boxed my previous answers in case they are needed to figure out the four questions. I need help on the third page. The secon

Estimation of pH of solution based on color of 2 indicators

Please see the attached file for the fully formatted problems. 1. Estimate the pH of the following, based on the indicator colors given: Solution Tested Bromocresol Green (indicator color) Bromothymol Blue (indicator color) Estimated pH Distilled water Blue Yellow

How to write a chemistry lab report

A full lab report, including propagation of error, with instructions on what belongs in each section (abstract, introduction, experimental, results and discussion, acknowledgments, references, and appendices). This sample lab concerns the determination of the percent chloride in a soluble unknown, but has general notes for each

Using indicators to measure acidity

Please help with the following multiple choice questions regarding acids and bases. You have two neutral solutions. One contains the indicator methyl red, which turns red in strongly acidic aqueous solutions but is otherwise yellow. The other contains the indicator phenol red, which turns red in strongly basic aqueous soluti

Questions Regarding Equilibrium Reactions

1. Given the following reaction H2(g) + I2 (s) = 2HI (g) ¤h = + 68.0 KJ/mol A) Write the Kc expression. B) State whether the number of moles of H2 (g) in the container will increase, decrease, or remain the same after each of the following disturbances is applied to the original mixture. For each case, assume that al

pH and Ka of lactic acid

3. Lactic acid, HC3H5O3, is a monoprotic acid that dissociates in aqueous solution, as represented by the equation(not given). Lactic acid is 1.66 % dissociated in 0.50M HC3H5O3. (aq) at 298K. A) Write the expression for the acid- dissociation constant , Ka , for lactic acid and calculate its value. B) Calculate the pH

properties of HF and the strongest base in the reaction

5. When comparing 0.050M HF (aq) and 0.010M HF (aq) which of the following statements is false ? A. The pH of 0.050M is lower than the pH of 0.01M B. The percent ionization of 0.010M is greater than 0.050M C. The electrical conductivity of 0.050M is greater than 0.010M D. All of the above ( therefore the statements are

The Enthapy Change of a Chemical Reation involving Mg

Lab Tools : Thermometer, Balance Lab Glassware : Calorimeter Lab Chemicals : H2O, Mg, HCl Lab Background : When an exothermic reaction takes place in a container, heat is released and warms up the container and its contents. The contents of the container include the reaction products and a solvent (such as water), if

Acids, Bases, Titrations and Indicators

4) Aniline, a weak base, reacts with water according to the reaction represented above. a) Write the equilibrium constant expression, Kb, for the reaction represented above. b) A sample of aniline is dissolved in water to produce 25.0mL of a 0.10M solution. The pH of the solution is 8.82. Calculate the equilibrium constsant

pH of solution

Weak acid - strong base 50.0ml of 0.20 M HCOOH ( Ka = 1.8 x 10^-4) with 0.1 M NaOH A) what volume of NaOH will be added at equilibrium ? B) what is the initial pH ? C) between initial and equivalence point D) at equivalence point E) beyond equivalence point F) what happens exactly halfway to the equivalence po

buffered solution

Short answer: A) pH of a buffer is determined by : B) buffer capacity is determined by :

titration of hypochlorous acid using NaOH

5) Ka = [H3O+ ] [OCL ]. = 3.2 x 10^-8 ................................. [HOCL ] Hypochlorous acid , HOCl , is a weak acid in water with the above Ka A) write a chemical equation showing how HOCl behaves as an acid in water B) calculate the pH of a 0.175 M solution of HOCl C) write the

pH of the solution

4). calculate the pH of a 0.265 M solution of propanoic acid HC3H5O2 (aq) = C3H5O2- (aq) + H+ (aq), Ka = 1.34 x 10^-5 Propanoic acid ionizes in water according to the equation above A) write the equilibrium- constant expression for the reaction B) calculate the pH of a 0.265 M solution of propanoic acid 5) A 0.496

Dissociation of HF in Water and Reaction with Strong Base

1. HF(aq) + H2O(l) <----> H3O+(aq) + F- (aq) Hydrofluoric acid dissociates in water as represented by the above equation With Ka = 7.2 * 10^-4 A) write the equilibrium- constant expression for the dissociation of HF(aq) in water B) calculate the molar concentration of H3O+ in a 0.4M HF solution HF reacts with NaOHaq ac

Draw the structure of the dye formed from Primuline red and 2-naphthol.

1) Discuss the results of your classification tests and melting point of your derivatives. What is your unknown? How do your data exclude other possibilities and what, if anything is still inconsistent with your conclusion? "Boiling Point for the Unknown is 218oC. For the 2,4-dinitrophenylhydrazone derivative of the unknown, th

Conductivity of acetic acid KCl solutions

The conductivity of a 0.1 moldm^-3 solution of potassium chloride at298K was found to be 1.1639 x 10^-2 Scm^-1. In a separate experiment at 298K the resistance of a 0.1 moldm^-3 solution of ethanoic acid was determined as 300 ohms and the resistance of the potassium chloride solution was fond to be 33.21 ohms. Given that the spe

Chemistry and Blood pH

Maintaining blood pH: the role and control of CO2 in blood buffering. Maintenance of blood pH is critical to life. Slight fluctuations of pH result in conditions of acidosis or alkalosis. The carbonate buffer system is a key factor in controlling the pH. In this assignment you are to combine several key concepts in explaining

Structural Formulae of Two Carbon Compounds

Please see the attachment for the figures. a) Figure 1 (overleaf) shows the abbreviated structural formulae of two carbon compounds (labelled A and B) and the reaction (Reaction 1) between them. The Equation for this reaction is incomplete; only the reactants are shown, and the missing product (s) is indicated by a question m

Amount of NaOH needed to Raise the pH of a Solution

A 2 part question ---- and the 2 parts are not inter-related: 1) I need to calculate the amount of NaOH (pH = 13.0) needed to raise the pH of a 3402 m3/minute wastewater flow from a pH of 4.3 to: a) a pH of 6.0 b) and/or pH of 7.0 2) I cannot find anywhere a vapor pressure for CO2 in water at higher temperatures....I

Total Pressure

For the reaction H2S(g) + I2(s) <-----> S(s) + 2 HI(g), the equilibrium constant Kp = 1.33e-05 at 333 K. What will be the total pressure of the gases in an equilibrium mixture if P(of)HI = 0.01 x P(of)H2S? (in atm) (Using correct significant figures)