A 2.5×10−2 M solution of HCl is used to titrate 147 mL of a Ca(OH)2 solution of unknown concentration. 1. If 100 mL of HCl is required, what is the normality of the Ca(OH)2 solution? Express your answer using two significant figures. 2. What is the molarity? Express your answer using two significant figures.
An aqueous solution of Ca(OH)2with a concentration of 0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid? What is the molarity of the original HCl solution? 04 Question (a points) aSee page 166 Watch the...
47 mL of 0.02M of HCl is used to titrate 25mL of Ca(OH)2. a) What is the molarity of the hydrochloric acid? b) What is the molarity of the hydroxide ions in the Ca(OH)2? c) Calculate the solubility product from the titration. Answer needs to be written using Engineering notation, where 3.14 x 10-5 = 3.14E-5.
An aqueous solution of Ca(OH)2with a concentration of 0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01× 10-14.) (a) What was the original pH of the ammonia solution? 匹の10.85 (b) What is the pH at the equivalence point? の5.50 (c) Draw a titration curve for this titration. ( r curve should be quantitative; calculate the pH at different points to construct...
It required 28.9 mL of 0.0170-M Ba(OH)2 solution to titrate a 25.0-mL sample of HCl to the equialence point. Calculate the molarity of the HCl solution. Molarity = M
Question 38 2.5 pts Suppose 19.2 mL of 0.489 M HCl was used to titrate an unknown sample of KOH (molar mass 56.11 g/mol). What mass of KOH was in the sample? The balanced chemical equation is: HCI + NaOH- NaCl + H20 O 0.114g O 0.527 g O 0.437 g 0 3.42 g
5.0 ml of saturated borax solution requires 12.77 ml of 1.0 M HCl solution to titrate it. What is the Ksp of Borax?
Calculate the molarity of a HCl solution if 25.0 mL of the solution is required to completely titrate 25.0 mL of 0.0400 M Ca(OH)2 • 0.0400 M 0.0800 M O 0.0200 M 4.00 10-5M O 0.220 M
Question 3 3 pts 3. A 2.5 M HCl solution is used to titrate (neutralize) a 5.0 M NaOH solution. a. How many ml of the HCI solution would be needed to "neutralize" 400 ml of the 5.0 M NaOH?? (think C1V1=C2V2) b. Write the balanced equation for the reaction of HCI with NaOH c. In the above equation which you just wrote, identify the conjugate acid and the conjugate base Upload Choose a File