mol NaOH=(0.00535L)(0.1M)=0.000535mol
mol HCl=(0.02L)(0.1)=0.002mol
mol HCl neutralized by antacid: 0.002mol -0.000535mol =0.001465mol
If 5.35mL of 0.1000 M NaOH solution is needed to just neutralize excess acid after 20.00...
If 6.00mL of 0.1000 M NaOH solution is needed to just neutralize excess acid after 20.00 mL of 0.1000 M HCl was added to 1.00 g of an antacid, how many moles of acid can the antacid counteract per gram?
If 5.70mL of 0.1000 M NaOH solution is needed to just neutralize excess acid after 20.00 mL of 0.1000 M HCl was added to 1.00 g of an antacid, how many moles of acid can the antacid counteract per gram?
What is the volume of 0.700 M NaOH needed to neutralize the 20.00 mL of 1.30 M HCl solution?
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...
A solution of malonic acid was standardized by titration with 0.1000 M NaOH solution. If 20.76mL of the NaOH solution were required to neutralize completely 12.95 mL of malonic acid soulution, what is the molarity of the malonic acid solution?
A) What is the volume of 0.700 M NaOH needed to neutralize the 20.00 mL of 1.30 M HC1 solution? b) The data suggest a different volume was needed to neutralize the HCI. Explain why this may be the case.
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...
2. In an acid-base titration, 25.62 mL of an NaOH solution are needed to neutralize 26.23 mL of a 0.1036 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: a. First note the value of M.. in the HCl solution. b. Find Mo- in the NaOH solution. (Use Eq. 3.) c. Obtain M Nach from Moh-- M
1) How many milliliters of a 0.100 M NaOH solution are needed to neutralize 15.0 mL of 0.200 M H₃PO₄? 2) If 24.7 mL of 0.250 M NaOH solution are needed to neutralize 19.8 mL of H₂SO₄, solution, what is the molarity of the H₂SO₄? 3) 25.0 g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?
2. In an acid-base titration, 25.62 mL of an NaOH solution are needed to neutralize 26.23 mL of a 0.1036 M HCI solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of M in the HCl solution. a. H* b. Find M Oн in the NAOH solution. (Use Eq.3.) from MOH NaOH c. Obtain M.