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 .....................................................................
5.Which of the following does NOT represent a conjugate acid/base pair A. HC2H3O2 / C2H3O2- B. HCN / CN- C. H3O+ / OH- D. HCL / CL- E. All are conjugate pairs Justify your answer and explain why the incorrect ones are false .......................................................................... 7. Which
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
Without doing detailed calculations, determine which of the following is the most likely pH for 0.010 M H2SO4. (a) 1.45 (b) 1.65 (c) 1.85 (d) 2.05 (e) 2.25 (f) 2.45
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 H3O^+ concentration in a 1.02 M solution of potassium nitrite (in mol/L).
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.
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 :
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
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
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
Please see the attachment for the figures. a) Figure 1 (overleaf) shows the abbreviated structural formulae of two carbon compounds (labelled A and B) and the reaction (Reaction 1) between them. The Equation for this reaction is incomplete; only the reactants are shown, and the missing product (s) is indicated by a question m
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)