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Acids and Bases

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

pH at the equilibrium point

6) When 12.0ml of 0.250 M NaOH is added to 10.0ml of 0310 M HCL, has equilibrium been reached? Explain. What is the pH at this point ?

buffered solution

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

pH of Buffer Solution: Sodium Lactate and Lactic Acid

1) A buffer is prepared by adding 0.200 mol of sodium lactate ( NaC3H5O3) to 500ml of 0.5 M lactic acid ( Ka = 1.4 x 10^-4). A) What is the pH of the buffered solution? B) What is the pH after 100ml of 0.100 M HCL is added to the buffer? C) What is the pH after 12 g of NaOH is added to the original solution prepared in

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

Neutralization of Acetic Acid with NaOH

Write a balanced equation for the neutralization of acetic acid with NaOH. I have actually gotten better at balancing equations---but I have no idea where to even start with this one. Any help you can provide would be greatly appreciated. Thank You,

pH of the aqueous solutions

What is the pH of each of the following aqueous solutions? (a) 0.0029 M HCl (b) 0.0050 M NaOH (c) 0.0013 M Ba(OH)2 (d) 1.2 x 10^-3 M HBr

Kb of Codeine - Calculating the K value

Codeine, C18H21NO3, a commonly prescribed painkiller, is a weak base. A saturated aqueous solution contains 1.00 g codeine in 120 mL of solution and has a pH = 9.8. What is the Kb of codeine? C18H21NO3 + H2O <----> [C18H21NHO3]^+ + OH^- Kb = ?

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

Calculating amount of H3PO4 to reduce pH of wastewater

Wastewater flow is 1.5 million gallons per day. The pH of the incoming wastewater is 5.2 The desire is to use 30% H3PO4 to reduce the pH of the wastewater to pH 2.5. How would I calculate the amount of 30% H3PO4 needed to accomplish this pH change for the 1.5 MGD wastewater flow??? Please show me your calculations.

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