Macmillan Learning equation: Write the balanced equation for the ionization of the weak base pyridine, C,H,N, in water, H₂O. Phases are optional.
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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.Consider the explanation in the Introduction regarding the determination of qrxn, and answer the following questions about the reactions that you will be performing in this experiment. Part A: If the temperature of the HCl solution increases, did the solution absorb heat or release heat? A.)Absorbed heat B.)Released heat C.)Neither absorbed nor released heat Part b: Consider the explanation in the Introduction regarding the determination of qrxn, and answer the following questions about the reactions that you will be performing in this experiment. Based on your answer to question 1, Will qsoln be a positive or negative quantity? A.)Positive B.)Negative C.)Zero Part C Consider the explanation in the Introduction regarding the determination of qrxn, and answer the following questions about the reactions that you will be performing in this experiment. Based on your answers to questions part A and B, If the temperature of the HCl solution increases, then did the reaction…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)
- Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go downThe 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.Can you please answer this and show a explanation.
- An aqueous solution of formic acid, that is 1.00 percent by weight formic acid, has a density of 1.0006 g/mL. A student determines that the freezing point of this solution is -0.418 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of Ka? Kf for H2O is 1.86 °C/m. % ionized = % Ka =A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour. Most of the coal burned in the United States contains 1 to 4 % by weight sulfur in the form of pyrite, which is oxidized as the coal burns: 4FeS2(s) + 11 O₂(g) 2 Fe2O3(s) + 8 SO2(9) Once in the atmosphere, the SO2 is oxidized to SO3, which then reacts with water in the atmosphere to form sulfuric acid: SO3(9) + H₂O(1)→→→→→→→ H₂SO4(aq) If 42.4 metric tons of coal that contains 1.44 % by weight S is burned and all of the sulfuric acid that is formed rains down into a pond of dimensions 397 m x 256 m x 4.96 m, what is the pH of the pond? (OK to assume 2 mol H30+ per mole H₂SO4.) Hint: 1 metric ton = 1000 kgUse the key below to answer questions 3a and 3b. HA A- H3O+ H2O Draw a picture to represent the molecular view of the dissociation of HNO3 in water. Draw a picture to represent the molecular view of the dissociation of HC2H3O2 in water.