What is the volume of an HCl solution which contains 0.032 moles of HCl and a pH of 1.54?
Calculate the pH of a 0.530 L HNO3 solution which fully neutralizes a 1.25 L LiOH solution with a pH of 8.4?
What volume of HNO3 solution at pH 1.07 is required to neutralize 15.0 mL of a 0.012 M Ba(OH)2 solution?
What is the volume of an HCl solution which contains 0.032 moles of HCl and a...
What volume of a 0.500 M HCl solution is needed to completely neutralize 10.0 mL of a 0.200 M Ba(OH)2 solution? Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2 H2O(l) a. 10.0 mL b. 4.00 mL c. 2.00 mL d. 8.00 mL
1) What is the volume of a 1.20 M HNO3 (aq) solution that contains 0.0420 moles of HNO3 ? 2) What is the volume (in mL) of a 0.125 M Ba(ClO4)2 solution that is needed, to completely react with 20.00 mL of 0.250 M K3PO4 solution according to the reaction below ? 3 Ba(ClO4)2(aq) + 2 K3PO4(aq) → Ba3(PO4)2(s) + 6 KClO4(aq)
1) what volume (in mL) of a 12.0M HCl (aq) solution contains 0.600 moles of HCl? 2) "concentrated" hydrochloric acid has a concentration of 12M. How many moles HCl are in 25 mL of conc. HCl?
What volume of 0.1292 M Ba(OH)2 would neutralize 50.00 mL of 0.1000 M HCl solution? Ba(OH)2(aq) + 2HCl(aq) ⟶ BaCl2(aq) + 2H2O(l)
1.) How many moles of NaOH (aq) are needed to neutralize 3.2 mol H2SO4(aq)? 2.) How many moles of Ba(OH)2 (aq) are needed to neutralize 3L of 0.8 M HCl solution? 3.) What is the volume of 0.5 M H2SO4 solution needed to neutralize 0.15 L of 0.6M NaOH solution? 4.) How many grams of NaOH needed to neutralize 0.25 L of 0.6 M H2SO4 solution? Molar mass of NaOH= 40 g/mol 5.) 2.8g of Ba(OH)2(s) is added to water...
1- Calculate the molarity of a HCl solution that contains 44.2 g of HCl in a total of 1250mL of solution. 2- How many mL of a 0.350 M LiOH solution contain 0.0171 moles of LiOH?
It is titrated with 0.1 M HCl 25 mL of a solution which contains a mixture of salts: NaHA and Na2A. Two points are known from the valuation curve: 1) when adding 1.25 mL of HCl the pH is 6.0 and 2) Add 12.5 mL of HCl the pH is 4.5. Calculate the volume of the 0.1 M HCl solution necessary for the complete evaluation of both salts H2A (pKa1 = 3.0, pKa2 = 6.0). ANSWER 35 mL
What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.65 L of an HCl solution with a pH of 1.9?
2. Consider the following two solutions: Solution A has a volume of 1 litre which contains 0.35 moles of acetic acid and 0.25 moles of sodium acetate. The Ka value for acetic acid 1.78 * 10". Solution B also has a volume of 1 litre and it contains 2.8 * 10* mol HCl and 2.84 * 10-4 mol of NaCl. a) Calculate the pH of each of the two solutions. b) What is the pH of each solution after thoroughly...
What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.60 L of an HCl solution with a pH of 1.60? Express your answer to two significant figures and include the appropriate units.