100 mL of 0.1 M HCl are mixed with 100 mL of 0.25 M NaOH. If the temperature of solution rose 5.0 degree C, what is the heat of reaction? Heat lost by_____ = - Heat gained by _____
100 mL of a 0.2 M solution of NaOH is mixed with 150 mL of a 0.3 M HCl solution. A neutralization reaction occurs: NaOH + HCl —> NaCl + H2O. What is the molarity of the molecules in the mixed solution after the reaction has reached completion?
100 mL of 0.500 M HCl is mixed with 100 mL of 0.600 M NaOH in a constant pressure calorimeter. The initial temperature of the solutions is 22.50 C and the final temperature of the mixed solution is 25.86 C. Calculate ?rH (in units of JK/mol-rxn) for the reaction NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l) The density of the resulting solution is 100 g/mL, and its specific heat is 4.184 J/(g C). Thank you in advance!
When 50ml of 0.10M HCl is mixed with 50 ml of 0.30M NaOH, what is the approximate pH of the resulting solution? When 50 mL of 0.10 M HCI is mixed with 50 mL of 0.30 M NaOH, what is the approximate pH of the resulting solution? (B) 7 (C) 9 (A) 1 E) 13 ** (D) 11 . *
1. What volume of 0.10 M NaOH is needed to neutralize 100 mL of 0.050 M HCl? 2a. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.01 M of HNO3 solution, what is the concentration of H+ and the pH in the resulting mixture? 2b. When 100 mL of 0.01 M NaOH solution is mixed with 100 mL of 0.02 M of HCl solution, what is the concentration of H+ and the pH in...
If 5.0 mL of 0.1 M NaOH is added to 50.0 mL of 0.1 M HCl, what will be the resulting pH of the solution? Round your answer to the tenths place. Do not include units in your response.
(e) Consider this example problem: If 100 mL of 0.100 M HCl solution is mixed with 100. mL of 0.100 M NaOH, what is the molarity of the resulting salt solution? (assuming the volumes are additive and ignore the change in H2O, which is negligible). HCIA NaOHa NaCl + H2O 1 mol 1 mol 1 mol Mols @Start: 100 mL (100 M ME!) 100 ml (0.1.000 ) O mol = 10 mmol HBr = 10 mmol NaOH Change - 10...
2. What is the "What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M HCl and 30.00 mL of 0.125 M NaOH? We assume additive volumes. 3. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (K, for acetic acid is 1.8x10-5.)
The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc- is a weak base. Ka for acetic acid = 1.75 * 10^-5. a) Calculate the pH of the 50.0 mL of 0.1 M OAc- solution before the addition of any HCl. b) Calculate the pH of the resulting solution after the addition of 5.0 mL of 0.2 M HCl to the 50.0 mL of 0.1 M OAc- solution. c) Calculate the pH of the resulting...
If you titrated 30.0 mL of 0.1 M HCl with 0.1 M NaOH indicate the approximate pH at... a.) the start of the titration b.) at the equivalence point c.) What is the total volume of the solution at the equivalence point?