Calculate the expected change in temperature for 25.00 mL of 0.500 M HCl reacting with 25.00...

Calculate the expected change in temperature for 25.00 mL of 0.500 M HCl reacting with 25.00 mL of 0.500 M NaOH. The heat Capacity of the Calorimeter is 15.6 J C -1 and the molar Enthalpy of Neutralization is -55.83 kJ mole . (Remember to use -1 dimensional analysis)

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

For the titration of 25.00 mL of 0.1000 M HCl with 0.1000 M NaOH, calculate the...

For the titration of 25.00 mL of 0.1000 M HCl with 0.1000 M NaOH, calculate the pH of the reaction mixture after each of the following total volumes of base have been added to the original solution. (Remember to take into account the change in total volume.) Select a graph showing the titration curve for this experiment. (a) 0 mL (b) 10.00 mL (c) 24.90 mL (d) 24.99 mL (e) 25.00 mL (f) 25.01 mL (g) 25.10 mL (h) 26.00...

25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this...

25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this the titration solution after the addition of a) 12.5 mL and b) 25.00 mL of the titrant has been added. Based on these pH values, select an appropriate indicator for the titration from table at the end of lecture notes for Chapter 16.

Consider the titration of 40.00 mL of 0.200 M NH3 with 0.500 M HCl. Calculate pH...

Consider the titration of 40.00 mL of 0.200 M NH3 with 0.500 M HCl. Calculate pH a) initially b) after addition of 5.00 mL of 0.500 M HCl c) at the half-neutralization point (halfway to equilvalence point) d) after the addition of 10.00 mL of 0.500 M HCl e) at the equivalence point

Calculate the pH of each of the following mixtures. a) 25.00 ml 0.2875 M HCl mixed...

Calculate the pH of each of the following mixtures. a) 25.00 ml 0.2875 M HCl mixed with 12.25 ml 0.3548 M KOH b) 25.00 ml 0.2875 M HCl mixed with 35.25 ml 0.3548 M KOH c) What is the pH of a solution containing 0.52 M HBr and 1.25 M CH3CO2H. d) 25.00 ml 0.2875 M HOCl (ka = 3.5 x 10-8) mixed with 12.25 ml 0.3548 M KOH e) 25.00 ml 0.2875 M HOCl (ka = 3.5 x 10-8)...

If 85.00 mL of 0.100 M HCl is mixed with 25.00 mL of 0.200 M H2SO4...

If 85.00 mL of 0.100 M HCl is mixed with 25.00 mL of 0.200 M H2SO4 and 50.00 mL of 0.400 M NaOH. What is the resulting pH of the final solution? Please show all work and how the formulas are derived if modified.

9) An aqueous solution of HCl is 0.500 M. Its density is 1.20 g/mL. Calculate the...

9) An aqueous solution of HCl is 0.500 M. Its density is 1.20 g/mL. Calculate the molality of HCl in this solution. a) 0.417 m b) 0.424 m c) 0.430 m d) 0.500 m e) 0.600 m 10) The normal freezing point of benzene (C6H6) is 5.48°C. When 2.00 g of an unknown covalent compound is dissolved in 100.0 g of benzene, the freezing point of the resulting solution is 5.08°C. What is the molar mass of the unknown compound?...

calculate the pH for the titration 20 mL of 0.500 M HF with 0.500 M KOH...

calculate the pH for the titration 20 mL of 0.500 M HF with 0.500 M KOH at the following volumes ka, HF is 6.8E-4 using the Rice table a.0 mL b.10 mL c.19 mL d. 20 mL e. 21 mL f. 30 mL

Calculate the pH change when 10. mL of 3.0 M HCl are added to 500. mL...

Calculate the pH change when 10. mL of 3.0 M HCl are added to 500. mL of the following A ) pure water B) aqueous solution of 3.0g of formic acid C) aqueous solution of 4.0g potassium formate D) aqueous solution containing 3.0 g of formic acid and 4.0 g of potassium formate

1.How many mL of 0.500 M HCl should be added to 155 mL of 0.0500 M...

1.How many mL of 0.500 M HCl should be added to 155 mL of 0.0500 M benzylamine to form a buffer with pH = 8.52? C7H7NH2 pKb = 4.35 C7H7NH2 (aq) + H+ (aq)  C7H7NH3 + (aq) This structure of benzylamine has a carbon at the junction of each line with 1 hydrogen on each 3-bonded ring C and 2 hydrogens on the C in the side chain attached to the ring carbon. Note that the N atom has...

Calculate the pH change when 5.0 mL of 5.0-M NaOH is added to 0.500 L of...

Calculate the pH change when 5.0 mL of 5.0-M NaOH is added to 0.500 L of a solution of: (The pKa for acetic acid is 4.74.) a) 0.50-M acetic acid and 0.50-M sodium acetate. pH change = _____ b) 0.050-M acetic acid and 0.050-M sodium acetate. pH change = ______ c) 0.0050-M acetic acid and 0.0050-M sodium acetate. pH change = _______

Subjects