What is the concentration of NaOH solution (M) if you have the mass of NaOH as 0.12 grams and the volume as 250.00 ml ?...
What is the concentration of NaOH solution (M) if you have the mass of NaOH as 0.12 grams and the volume as 250.00 ml ? The PH of the solution is 11.5
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What is the concentration of NaOH solution (M) if you have the mass of NaOH as 0.12 grams and the volume as 250.00 ml ?...
We have (a) 50.0 mL of 0.10 M NH3 solution, (b) 50.0 mL of 0.12 M...
We have (a) 50.0 mL of 0.10 M NH3 solution, (b) 50.0 mL of 0.12 M HNO3 solution, (c) 50.0 mL of 0.12 M NaOH solution, and (d) 50.0 mL of 0.06 M HClO4 solution. Can you make a buffer by combining two of these solutions? If so, which ones? What would be the pH of the buffer solution? Please explain
#1. If you have 250. mL of a buffer that is 0.12 M in H2PO4- and...
#1. If you have 250. mL of a buffer that is 0.12 M in H2PO4- and 0.12 M HPO42- , what will be the pH after 27.77 mL of 0.193 M NaOH is added? Ka2 is 6.21 x 10-8 . #2. Given 1000. mL of a 0.434 M solution of C2H5NH2 (pKb = 3.19), what is the pH if 26.45 g of C2H5NH3Cl (81.5446 g/mol) are added?
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL...
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL volumetric flask and dilutes up to the mark with distilled water. What is the final molarity of the dilute solution? Select one: A. 0.1 MX B. 0.10206 M C. 0.102 M D. 0.1021 M Your answer is incorrect. 86.14 mL of an acid solution was needed to neutralize 30.24 mL of a base solution of unknown concentrations. A second trial is run but this...
Mass of Unknown: 873 NaOH Concentration 0-1349 M Volume NaOH Average NaOH used (mL) Volume (mL)...
Mass of Unknown: 873 NaOH Concentration 0-1349 M Volume NaOH Average NaOH used (mL) Volume (mL) Run # 117m 1/. 067mL 9.7mし Be sure to show ALL of your work Determine the number of moles of unknown acid in your 25 mL sample-Show Calculations
1. What volume of 0.10 M NaOH is needed to neutralize 100 mL of 0.050 M...
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...
What is the resulting pH when you combine 75.0 mL of a 0.12 M solution of...
What is the resulting pH when you combine 75.0 mL of a 0.12 M solution of NaOH and 83.0 mL of a 3.9 M solution of acetic acic acid has a Ka = 1.8 x 10-5. HINT: Find the concentrations first, then plug into an ice table. Make sure you know the total volumel
Concentration 1.00 M of NaOH Volume of Solution 2.5 mL added to solution 4.0 mL added...
Concentration 1.00 M of NaOH Volume of Solution 2.5 mL added to solution 4.0 mL added to solution 2.00 M of Caci, 2.0 mL added to solution 0.75 M of K,POL Each of these three solutions are mixed into a beaker, find the molarity of each of the three individual solutions in the entire solution.
Draw the titration curve for the titration of 20 mL of a 0.12 M solution of...
Draw the titration curve for the titration of 20 mL of a 0.12 M solution of glutamate (carboxylic acid pKa = 2.19, amino pKa = 9.67, you need to know the pKa for the R group) with 0.10 M sodium hydroxide. Clearly label the axes of your graph (pH vs mL of NaOH added.) Be sure to include pH values and volumes for the following: Start of the titration (no sodium hydroxide added), the pH at the volume that is...
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What...
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass = g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What...
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass = g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL volumetric flask and dilutes up to the mark with distilled water. What is the final molarity of the dilute solution? Select one: A. 0.1 MX B. 0.10206 M C. 0.102 M D. 0.1021 M Your answer is incorrect. 86.14 mL of an acid solution was needed to neutralize 30.24 mL of a base solution of unknown concentrations. A second trial is run but this...
Mass of Unknown: 873 NaOH Concentration 0-1349 M Volume NaOH Average NaOH used (mL) Volume (mL) Run # 117m 1/. 067mL 9.7mし Be sure to show ALL of your work Determine the number of moles of unknown acid in your 25 mL sample-Show Calculations
What is the resulting pH when you combine 75.0 mL of a 0.12 M solution of NaOH and 83.0 mL of a 3.9 M solution of acetic acic acid has a Ka = 1.8 x 10-5. HINT: Find the concentrations first, then plug into an ice table. Make sure you know the total volumel
Concentration 1.00 M of NaOH Volume of Solution 2.5 mL added to solution 4.0 mL added to solution 2.00 M of Caci, 2.0 mL added to solution 0.75 M of K,POL Each of these three solutions are mixed into a beaker, find the molarity of each of the three individual solutions in the entire solution.
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass = g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass = g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M
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