2. A buffer can be prepared by adding strong acid to excess weak base or by adding a strong base to excess weak acid. Please explain.
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
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 ?
5). What mass of NaOH must be added to a 0.200 M HF (aq) to prepare a buffer with a pH of 3.0?
Short answer: A) pH of a buffer is determined by : B) buffer capacity is determined by :
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
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
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
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
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
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,
1. The differences in Arrhenius, Lowry-Bronsted, and Lewis theories of acids and bases are important in recognizing where they are applied. Where are each of these theories applied in Chemistry? 2.pH is the controlled process of digestion, bleaching, creating of pulp to manufacture of finished paper products. How do they mea
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
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 = ?
Formic acid, HCOOH (Ka = 1.8 x 10^-4), is the irritant associated with ant stings. Calculate the pH of an aqueous solution 80.6 g HCOOH per liter.
Calculate the pH of 0.211 M CCl3COOH (trichloroacetic acid, pKa = 0.52).
The pH of a cup of coffee at 25 degrees Celsius is 4.39. What is the [H3O^+] in the coffee (in M)?
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
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.
Identify the following as either Ionic or Covalent Compounds: 1. Potassium bromide 2. Lithium carbonate 3. Magnesium nitrate 4. Phosphoric A
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 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
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
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)
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)
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?
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
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
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
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