If 2.00 mL of 0.300 M NaOH are added to
1.000 L
of
0.400 M CaCl2,
what is the value of the reaction quotient and will precipitation occur
If 2.00 mL of 0.300 M NaOH are added to 1.000 L of 0.400 M CaCl2,...
Be sure to answer all parts. If 2.00 mL of 0.250 M NaOH are added to 1.000 L of 0.100 M CaCl, what is the value of the reaction quotient and will precipitation occur? Q= x10 (Enter your answer in scientific notation.) Precipitation will not occur. O Precipitation will occur.
Calculate the pH of the resulting solution if 30.0 mL of 0.300 M HCl(aq) is added to (a) 40.0 mL of 0.300 M NaOH(aq). Number pH= 12.63 (b) 20.0 mL of 0.400 M NaOH(aq). Number pH= 1.22
Calculate the pH of the resulting solution if 30.0 mL of 0.300 M HCl(aq) is added to (a) 40.0 mL of 0.300 M NaOH(aq). Number pH= 12.63 (b) 20.0 mL of 0.400 M NaOH(aq). Number pH = Tools x 102
You add 2.00 mL of 0.400 M NaOH to 50.00 mL of pure water, and to this mixture you then add 15.00 mL of 0.800 M HCI. What will be the pH of the resulting solution?
Effect of Base on a Buffer vs. Water What is the pH if 5.00 mL of 4.0 M NaOH is added to 1.000 L of water. Pearson Copyright 2018, 2015, 2012 Pearson Education, Inc. All Rights Reserved 18
100.0 mL of 0.400 M aqueous NaOH and 50.00 mL of 0.400 M aqueous H2SO4, each at 24.00°C, were mixed, see equation: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) The final temperature achieved by the solution was 26.65 °C. Neglect the heat capacity of the cup and the thermometer, and assume that the solution of products has a density of exactly 1.00 g/mL and specific heat capacity of 4.18 J/(g•C) How much heat did the reaction release?
A 20.0-mL sample of 0.400 M HBr solution is titrated with 0.400 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added. (a) 11.6 mL (b) 15.7 mL (c) 20.0 mL (d) 28.2 mL (e) 33.1 mL
A 100.0 mL sample of 0.400 mol L-1 HCl(aq) is added to 150.0 mL of 0.300 mol LNH3(aq) (which can be thought of as a solution of NH4OH) in a coffee cup calorimeter and the temperature of the resulting solution rises from 23.92°C to 26.07°C. HCl(aq) + NH,OH(aq) → NH.Cl(aq) + H2O(1) (a) Determine the limiting reagent. (b) Calculate the enthalpy change, A.H.
You titrate 50.0 mL of 0.400 M HClO4 (a strong acid) with 0.400 M NaOH. a. Write the balanced equation. b. What is the pH at the beginning of the titration (0.0 mL of NaOH)? c. What is the pH after adding 30.0 mL of NaOH? d. At the equivalence point, is the pH greater than, less than, or equal to 7.00? Explain briefly.
How many milliliters of 0.250 M NaOH are required to neutralize 55.0 mL of 0.300 M H2SO4? The balanced neutralization reaction is: H2SO4(aq) +2 NaOH(aq) → Na2SO4(aq)+2H2O(l).