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
17. Using the following Ka values , indicate the correct order of of the conjugate base strength HNO2. Ka = 4.0 x 10-4 HF. Ka = 7.2 x 10 -4 HCN. Ka = 6.2 x 10-10 A. CN- > NO2- > F- > H2O > CL- B. CL- > H2O > F- > NO2- > CN- C. CN- > F- > NO2- > CL- > H2O D. H2O > CN- > NO2- > F- > CL- E. None of the ab
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
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
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
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
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
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.
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
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
Modeling the number of homes built over a period of time as an exponential function and logarithmic formula describing the PH of a substance.
Part 1: Suppose that the number of new homes built, H, in a city over a period of time, t, is graphed on a rectangular coordinate system where time is on the horizontal axis. Suppose that the number of homes built can be modeled by an exponential function, H= p * at , where p is the number of new homes built in the first year
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)
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
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
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.
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
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