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- A 0.109 mol/kg aqueous solution of formic acid, HCOOH, freezes at −0.210 °C. Calculate the percent dissociation of formic acid.In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO, (aq) + H,O(1) = H,O*(aq) + CI0, (aq) H,CO, (aq) + H,O1) – H;O*(aq) + HCO; (aq) Answer Bank H,O(1) + CH;NH†(aq) = CH,NH,(aq) + H;O*(aq) СА А B СВ CH, COOH(aq) + H,O(1) - CH;COO (aq) + H;O*(aq)The enthalpy change for the dissolution of sulphuric acid in water is -75.0kJ/mol. Concentrated sulphuric acid is an 18.1M solution. Calculate how much the temperature of the solution would change if you were making 1.38L of pH -0.56 H2SO4. Assume the solution has the same heat of solution as water, 4.186 kJ/Kg °C and the density of concentrated H2SO4 is 1.840 kg/L. Only your final answer is required to three sig figs.
- Answer the following by selecting all correct answers. (a) Dynamic equilibrium O is a condition where two opposing processes are occurring at the same rate. O can only occur in water. O is used to describe what happens when weak acids or weak bases are added to water. O is used to describe what happens when strong acids or strong bases are added to water. (b) What will happen if acetic acid (HC2H3O2) is added to water?Arrange the following bases in increasing base strength. There Strongest base Methylamine (CH3NH2), K, = 4.4 x 104 I Pyridine (C5H5N), K 1.7x 109 Aniline (C,H5NH2), K = 3.9 x 10 10 Dimethylamine (CH3)2NH), Kp = 5.1x 104 | Hydrazine (N2H4), Kg = 1.3 x 106 Weakest base 1. 2) 3. 4) 5.Can you please answer this and show a explanation.
- 6. A solution contains 0.67 M hydrofluoric acid (HF) and (15.0 x10³ M hydrochloric acid (HCI). Calculate the degree of ionization of hydrofluoric acid in the presence of hydrochloric acid. The K₂ of hydrofluoric acid (HF) at 25 °C is 3.2 x104. (9A solution of ammonium sulfate was prepared by dissolving 55.44g of (NH4)2SO4 in enough water to prepare a 2.00L solution. What is the concentration of ammonium ions in this solution?24. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?
- (a) Ionic Solids do not dissolve in non-polar solvents. (TRUE OR FALSE) (b) H3AsO4 is a weak acid. (TRUE OR FALSE) (c) Once a chemical reaction has come to equilibrium, the reaction comes to a complete halt.(TRUE OR FALSE)(6) Calculate the numbeT of moles of HNO, reacting when 50.0 mL of 1.00M HNO, and 50.5 mL of 1.00M NaOH solution are mixed. (7) Calculate AHneutza in joules per mole for the reaction of 1.00 mol of HNO3 with 1.00 mol of NaOH. (8) On the basis of an accepted AHneutzn of 58.5 kJ mol' for the reaction, determine the percent error in your calculated AHneutan. +Write a neutralization reaction for each acid and base pair. HBr(aq)and KOH(aq) Express your answer as a balanced chemical equation. Identify all of the phases in your answer.