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
13. Which of these salts will be more soluble in 0.10M HCL than in pure water A. PbCL2 B. NH4I C. CuBr D. Zn(HCO3) E. None of the above Explain your answer .......................................................................................................... 14. HA is an acid with a Ka = 1 x 10-5. What is
9. Silver chloride has a negligible solubility in water. It will dissolve in which of the following solutions A. C2H5OH (l) B. NaOH (aq) C. HNO3 (aq) D. NaCL (aq) E. NH3 (aq) Justify your answer and explain why the incorrect ones are false .....................................................................
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
If 2 mmol of the sodium salt of methyl salicyate are formed, how much many ml of 3M H2SO4 are needed to form salicylic acid? Assume 2 equivalents are needed. Can you explain to me how I figure out how much acid I need? I appreciate your help.
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
Use the Henderson-Hasselbalch equation to estimate the pH of the following buffer solutions prepared from hydrofluoric acid (in the following referred to as ACID) and sodium fluoride (referred to as SALT). (a) Put 7.282 g of ACID and 32.10 g of SALT into a volumetric flask, and fill with water to the 1 L mark. (b) Put 7.282
Citric acid (pKa1 = 3.13, pKa2 = 4.76, pKa3 = 6.40) is found in citrus fruit. Calculate the approximate pH of lemon juice, which is about 5% citric acid by mass.
Compute the pH of a 1.82 M solution of potassium nitrate.
Compute the H3O^+ concentration in a 1.02 M solution of potassium nitrite (in mol/L).
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.