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- A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
- . How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?Give typed explanation not written Consider the following Ka values for phosphoric acid, H3PO4.Ka1 = 7.1 x 10-3Ka2 = 6.3 x 10-8Ka3 = 4.2 x 10-13a.) What is the pH of a 4.0 M solution of H3PO4? b.) Determine the effectiveness of H2PO4acting as a base by calculating its Kb. c.) What is the pH of a 4.0 M solution of Na3PO4 (not H3PO4)?8) Determine the pH of the following solutions: a) 0.20 M CH3COOH b) 0.025 moles of CH3NH3CI dissolved in 1.50A102 mL of water c) 0.15 M solution of Cr(NO3)3 d) 0.25 M NazCO3 pKa of Cr+ is 3.89
- An analytical chemist is titrating 196.9 mL of a 0.1800M solution of piperidine (C-H₁0NH) with a 0.2000 M solution of HNO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 209.3 mL of the HNO3 solution to it. b Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0HC2HO3 (aq) _ H2O (l) <--> H3O+ (aq_ + C2HO3- (aq) pKa =3.18 at 25C The equilibrium for the acid ionization of HC2HO3 is represented by the equation above. If 10.0 mL of 0.20 M HC2HO3 react with 5.0 mL of 0.10M NaOH, how could you calculate the pH of the resulting solution?NTH assign one of the Trials to pe iment. Upon completion of your exper Volume (mL) 7.0 NICI₂6 H₂O mass of Nicl₂ •64₂0= 2.80 volume of 4.0 M C₂ 48 W₂ = 7.5 1 7.5 mass of witch glass 29.7189 mass of prodiect & watch ghasi 31.9739 mass of the product: 2.269. the pH is a light green & a 7 on the scale. Tria (3) shade. 0 the beaker until you obtai ation of the solid. filtrate in filter blask is pick- Lavener so C₂ 48 No is the excers reasent opwise to the solid unti mL. Record your obses 10 mL graduated cyli 7. Pour tion beaker, dropwise to the bea all of the solution, ges observed dur Ni Cl₂ · 6 Fl₂0 was the lumiting vergent. sti da second 5 mL aliquot RECOVE AL beaker th the ace ted cyli the be 5 mL aliquot of acetone to the
- Molecule A is C6H9O2F and an aqueous solution of 0.0130 M of molecule A has a pH of 1.0 . Calculate the pKa. Use at least 2 sig figs and no scientific notation.An analytical chemist is titrating 106.0 mL of a 0.1800M solution of piperidine (C5H₁NH) with a 0.7800M solution of HIO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 15.4 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = X B Ar. Describe the method to determine whether an amphoteric compound is acidic or basic given a table of Ka values. Table 2. Prediction of acidity and basicity ConcentrationActual (M) Compound pH ka kb 3.00E-5.56E- Pb(CH3COO)25.00E-03 5.3 08 10 5.60E-1.50E- NH4CO3 8.2 10 04 2.30E- 08 5.00E-03 NaHCO3 5.00E-03 9.0 6.40E-5.90E- |NaHSO3 5.00E-03 5.0 08 13
