Question 3 If you dilute 25.00 mL of 0.90 M sodium phosphide solution to make 75.00...
I have a 0.125 M sodium oxide solution a) 15.25 mL of this is diluted to 100.00 mL total volume. What is the concentration of the new solution? b) I now want to make 75.00 mL of a 20.00 mM solution. What volume of the 0.125 M solution must be diluted to 75.00 mL to make this? c) What is the concentration of sodium ions in the 0.125 M sodium oxide solution?
if 25.00 ml of 0.275 M solution of AgNO3(aq) is mixed with 25.00 ml of 0.300 M CaCl2(aq), what will be the reaction? What is the final concentration of all of the ions after the two solutions are mixed?
10 mL of a 0.30 M sodium phosphate solution reacts with 20 mL of 0.20 M lead(II) nitrate solution What mass of precipitate will form? What is the concentration of nitrate ions left in solution after the reaction is complete? What is the concentration of phosphate ions left in solution after the reaction is complete?
5. you take 25.27 mL of a 0.572 M solution of K Cro, and dilute it by adding 95.03 ml of 0.217 MKCE solution, what is the molar concentration of potassium ions in the diluted solution?
Question 1: In the laboratory you dilute 3.33 mL of a concentrated 6.00 M hydrochloric acid solution to a total volume of 75.0 mL. What is the concentration of the dilute solution? M Question 2: You wish to make a 0.153 M hydroiodic acid solution from a stock solution of 3.00 M hydroiodic acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Thank-you!
A student needs to dilute a 0.30 M Pb(NO,), solution to make 59.0 mL of 0.22 M Pb(NO,).. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.30 M Pb(NO solution that is needed. mL TOOLS x10' Answer Bank 0.22 M 0.30 ml 0.22 ml. 59.0L 0.30 M 59.0 ml.
b. How would you prepare 225.0 mL of 1.33 M HCl from a 6.00 M stock solution? C. When 25.00 mL of 0.695 M HCl reacts with an excess of silver nitrate, will a precipitate form? Write the net ionic equation for this reaction. How many grams of precipitate can be theoretically obtained? d. What volume of 0.2500 M strontium hydroxide is required to completely react with 75.00 mL of 0.07942 M HCI? e. When 37.5 mL of 0.439 M...
Question 3 (1 point) You have 25.00 mL of a 0.1000 M sugar solution. How much water must be added to make a 0.01059M solution? O 236.1 ml O 2.65 ml 022.4 mL O O 211.1 ml O 26.5 mL Question 4 (1 point) You have 100.0 mL of a 0.2500 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it is now 0.3930M. How much water must have evaporated? 063.6...
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...
A 25.00 mL solution containing 0.035 M sodium acetate is titrated with a 0.098 M solution of HCl. How many milliliters of HCI are required to reach the endpoint? Answer CHECK A 25.00 mL solution containing 0.035 M sodium acetate is titrated with a 0.098 M solution of HCI. How many milliliters of HCI are required to reach the endpoint? Answer: CHECK