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5. Indicate the mols present in the following solution: a) 0.25 M Baci2 in 1 liter b) 0.25 M C2H5OH in 0.5 liter c)...
6. Calculate the following quantities: a) milliliters of 0.75 M HCl required to neutralized completely 25.0 ml of 0.15 M Ba(OH)2 b) if 30.0 ml of 0.75 M HCl solution is needed to neutralize a 45 ml solution of Ca(OH)2, what is the concentration of Ca(OH)2 in the solution?
(0) How many milliers of 0.155 M HCl are needed to neutralize completely 45.0 ml of 0.101 M Ba(OH)2 solution? ml (b) How many milliliters of 2.50 M H2SO4 are needed to neutralize 25.0 9 of NaOH? (c) If 54.8 ml of BaCl solution is needed to precipitate all the sulfate in a 544 mg sample of Na2SO4 (forming Basod), what is the molarity of the solution? (d) If 37.5 mL of 0.250 M HCl solution is needed to neutralize...
4.82 (a) How many milliliters of 0.120 M HCI are needed to com- pletely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution? (b) How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.200 g of NaOH? (c) If 55.8 mL of a BaCl2 solution is needed to precipitate all the sulfate ion in a 752-mg sam- ple of Na2SOs, what is the molarity of the BaCl2 solution? (d) If 42.7 mL of 0.208 M HCl solution is needed...
(a) How many milliliters of 0.155 M HCl are needed to neutralize completely 35.0 mL of 0.101 M Ba(OH)2 solution? (b) How many milliliters of 2.50 M H2SO4 are needed to neutralize 75.0 g of NaOH? (c) If 56.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 554 mg sample of Na2SO4 (forming BaSO4), what is the molarity of the solution? (d) If 47.5 mL of 0.250 M HCl solution is needed to neutralize a...
A. How many milliliters of 0.110 M HCl are needed to completely neutralize 55.0 mL of 0.107 M Ba(OH)2 solution? Express the volume in milliliters to three significant digits. B. How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.170 g of NaOH? Express the volume in milliliters to three significant digits. C. If 55.0 mL of BaCl2 solution is needed to precipitate all the sulfate ion in a 746 mg sample of Na2SO4, what is the molarity of the solution? Express the molarity...
How many milliliters of a 0,40 M solution of hydrochloric acid (HCI) are necessary to neutralize 33 mL of a 0.20 M barium hydroxide (Ba(OH)2 solution? 16.5 mL 20 ml 66 mL O 33 mL O 10.5 mL
(1) For the following pairs of aqueous solutions: (1) KOH(aq) & Ag(NO3)2 (aq) (2) Ba(OH)2 (aq) & Pb(NO3)2(aq) Do the following: (a) Determine if a precipitate forms when the two solutions are mixed. (b) If a precipitate forms write down its molecular formula. (C) Write the net ionic equation for the precipitation reactions. (2) For the acid-base neutralization reactions below. (1) HCI + LiOH (2) HNO, + Ca(OH), Write down the: (a) Molecular equation (b) Net ionic equation (3) Compute...
REVIEW&CHECK FOR SECTION 4-5 1. A 1.71-g sample of Ba(OH)2(s) was dissolved in water to give 250 mL of solution. What is the OH concentration in this solution? (a) 0.010 M (b) 0.040 M (c) 0.080 M (d) 0.10 M 2. You have a 100.-mL volumetric flask containing 0.050 M HCI. A 2.0-mL sample of this solution was diluted to 10.0 mL. What is the concentration of HCl in the dilute solution? (a) 0.10 M (b) 0.010 M (c) 1.0...
A 25.0 ml solution of HNO3 is neutralized with 28.5 mL of 0.250 M Ba(OH)2. What is the concentration of the original HNO, solution? 16 O of 1 point earned 2 attempts remaining The pH of a 0.0030 M solution of Ca(OH)2 is O of 1 point earned 2 attempts remaining What volume (in mL) of 8.84 M HBr would be required to make 300.0 of a solution with a pH of 3.43? 18 0 of 1 point earned 2...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...