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    Acids and Bases

    Ionic and Convalent Compounds

    Identify the following as either Ionic or Covalent Compounds: 1. Potassium bromide 2. Lithium carbonate 3. Magnesium nitrate 4. Phosphoric A

    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

    The pH's of Eight 0.1 M Aqueous Salt Solutions

    The pH's of eight 0.1 M aqueous salt solutions are given below. Write the hydrolysis equation(s) for each. (Several will have more than one equation). If no hydrolysis reaction takes place,write N.R. Salt Solution pH a) Sodium Acetate 9 b) Sodium Carbonate 11 c) Ammonium Chloride 5

    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 in an equilibrium mixture

    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)

    activation energy of acetonedicarboxylic acid decomposition

    The rate constants for the first-order decomposition of acetonedicarboxylic acid is k1 = 3.54e-05 s^-1 at 274 K and k2 = 0.00128 s^-1 at 301 K. CO(CH2COOH)2 (aq) ----> CO(CH3)2 (aq) + 2CO2 Acetonedicarboxylic acid Acetone What is the activation energy, Ea, of this reaction? (in kJ/mol)

    Molarity and Molality

    A typical commercial-grade phosphoric acid is 75% H3PO4, by mass, and has density d= 1.57 g/mL. What are the molarity and molality of H3PO4 in this acid?

    Freezing point of naphthalene and benzene mixture

    How many grams of naphthalene, C10H8, would you add to 49.5 g of benzene, C6H6 (l), to produce a solution that has the same freezing point as pure water? (Use the data from the table as needed.) Molal Freezing Point Depression and Molal Boiling Point Elevation Constants: Solvent Normal Freezing K(fr) Normal

    Calculations with Acids and Bases

    I) Which one of these is the solute and which one is the solvent in a solution composed of i) 25.0 g of silver in 5.0 g of mercury, and ii) 3.0 g of iodine (I2) in 100.0 mL of ethanol? ii) What is it that makes water such a good solvent for polar substances? Why is it called the universal solvent? iii) What is the mass pe

    What is the concentration of Fe2+ (mol/L) in equilibrium with Fe(OH)3 ?

    At pH 6.00 and pE 2.50, what is the concentration of Fe2+ (mol/L) in equilibrium with Fe(OH)3? Hint: Use the Nernst equation and the Ksp for the solubility of solid iron (III) hydroxide. Note: I have already used the solution library examples and have come up with these wrong answers: 1.36e-3, 3.5e-3, 2.6645e-4, 2.9e-4, 5.495

    Resulting pH

    I am trying to figure this out but I don't have an measurement for water. Does that matter? Also, can I use the henderson hasselbalch equation to solve this? I need help with the setup of this problem. Thank you. In manufacturing a fruit drink, citric acid is added to water in the amount of 0.1 mol/L. What is the pH of the re

    An Estuarine Water Sample

    An analytical chemist determines that an Estuarine water sample contains 1.5 g/L of sulfate ion. What is the concentration in terms of: (a) g/L of S (b) molar concentration of sulfate (c) normality (d) parts per million of sulfate Could you please explain what formula and step are involved and please provide (example)

    pH of Resulting Solution

    In manufacturing a fruit drink, citric acid is added to water in the amount of 0.1 mol/L. What is the pH of the resulting solution? Could you please explain what formula and step are involved and please provide (example) problem

    Determining Concentration of a Compound when pH is Known

    We start with a 1 liter solution of water and a mild acid --- the pH of this solution is 4.0; To this solution, we add 100 grams of Chemical A that has a pH of 10.89 and a molecular weight of 300 g/mol; We then add 110 grams of Chemical B ---- Chemical B has a pH of 8.5 but its mol. wgt is unknown? We then add precisely

    Final pH of a Mixture of Acetic Acid, Alum, and NaOH

    A 1 liter solution of a mild acetic acid and water exhibits a pH of 4.0 --- the molar concentration of the acetic acid is unknown but is presumed to be 1x10^-4M; to this solution is added 100 grams of NaOH that has a pH of 12.0; then, 51 grams of aluminum sulfate hydrate (Al2(SO4)3-14H2O) with a pH of 3.5 is added to the solutio

    In this continuous process, "phosphoric acid and ammonia are mixed, and a non-hazardous product, diammonium phosphate (DAP) results if the reaction of ammonia is complete.

    Attached is a very simple process flow diagram. In this continuous process, "phosphoric acid and ammonia are mixed, and a non-hazardous product, diammonium phosphate (DAP) results if the reaction of ammonia is complete. If the proportion of phosphoric acid is reduced, the reaction is incomplete, and ammonia is evolved. Reduction

    Calculation of pH given Molarity

    I desperately need help with the following problems: Calculate the pH of the following solutions: a. a solution in which the H3O is 6.0 times 10 to the negative 6. b. 0.030 M of HI (aq) I need a step by step solution.

    Algal Bloom and Changes in pH

    Following an algal bloom, the pH of a lake increases from 7.3 to 10. If the pH is due to an increase in OH- ions via the reaction: HCO3 --> OH- + CO2, how many moles of OH- were released to raise the pH to 10?

    Strength of Acids

    Strength of acids makes a big difference on whether it is a mere sting or the dissolution of your cells. Would you rather have 1 mM of HCl on your skin or 0.1 M of HCl on your skin?

    Calculate the molarity and pH of the solution

    Mass of solute is given followed by the total volume of solution prepared. Calculate the molarity. a. 1.37 g of NaOH; 125 ml b. 4.29 g of Kl; 250. ml c. 2.95 mg of Pb(NO3)2; 4.95 ml d. 0.997 kg of NaNO3; 125 L What mass of the indicated solute does each of the following solutions contain. a. 2.50 L of 13.1 M HCl solutio

    Zinc Borate in Treatment of Wastewater

    Can you please take a look at the attached and give me some feedback. I want to understand why specifically pH is driven way low and then way high to promote precipitation of the zinc solids. Please take a look and comment. In our process, zinc borate (2ZnO-3H3BO3-3H2O) ultimately splits and dissociates to zinc oxide and b

    Solubility of Zinc Oxide, Boric Acid, and Aluminum Sulfate

    Hope you can help....I've always struggled calculating solubilities of compounds at different pH's. I have 3 separate but related questions: 1) 1000 g of zinc oxide is added to a 1 liter container of pH neutral water (pH 7.0); the solubility of the ZnO is given as .29 g/L at pH 7.0; how much more ZnO would dissolve if the pH

    Separating Sodium Carbonate, Chloride and Sulphate

    Assuming an imaginary mixture of sodium chloride, sodium carbonate and sodium sulphate I need to know what test to use to 1st confirm the the compostion and 2nd to find the percentage composition mixture. I need to know which test would be useful and the calaulations needed so I can preform the in the lab.

    'What Salt will Form', Precipitation and Reaction Type Problems

    When each of the following strong acid/strong base reactions take place. What salt would form with these and how would you find out. HCl (aq) + KOH (aq) --> RbOH (aq) + HNO (aq) --> HClO4 (aq) + NaOH (aq) --> HBr (aq) + CsOH (aq) --> How to Balance the following equations that describe combustion reactions. C2H6 (

    Determine the molar mass of an unknown acid.

    Please see attached file for full problem description. 1. Determine the molar mass of an unknown acid. Called the unknown acid HX, and it reacts with NaOH. Equation is: NaOH(aq)+HX(aq) --> NaX(aq)+H2O(l) 1 mole of NaOH reacts with 1 mole of HX. Weighed a sample of HX is titrated with standard NaOH. Weigh the vial contai

    Prediction of Changes to DeltaG in a Non-Standard Cell

    -438 kJ/mol is the free energy change of lactate oxidation by Fe3+ under non-standard conditions assuming that: C3H5O3- + 12 Fe3+ + 3 H2O -----> 3 CO2 + 11 H+ + 12 Fe2+ [Fe2+]=10^-4 M pH=7 T=25 degree centigrade [lactate]=10^-3 M Carbon dioxide is in equilibrium with atmospheric CO2 Fe3+ is in equilibrium with