7)
HNO3 + NaOH -------> H2O + NaNO3
1:1molar reaction
moles of NaOH consumed = ( 0.300mol/1000ml) × 15.4ml = 0.00462mol
0.00462moles of NaOH react with 0.00462moles of HNO3
moles of HNO3 present in 20.0ml solution = 0.00462mol
concentration of HNO3 = ( 0.00462mol/20.0ml)× 1000ml = 0.231M
8)
2H3PO4 + 3Ca(OH)2 ------> 6H2O + Ca3(PO4)2
stoichiometrically, 2moles of H3PO4 react with 3moles of Ca(OH)2
moles of H3PO4 consumed = ( 1.50mol/1000ml) ×15.65ml = 0.023475mol
0.023475moles of H3PO4 react with 0.035213 moles of Ca(OH)2
moles of Ca(OH)2 present in the 25.00ml solution = 0.035213mol
concentration of Ca(OH)2 = (0.035213mol/25.0ml) ×1000ml = 1.409M
7) Titrate 20.0 mL of HNO3 with an unknown concentration with 15.4 mL of 0.300M NaOH....
12. What is the concentration of the solution that results from diluting 75.0 mL of a 1.05 - solution of CH3OH to 500.0 mL? M. 1 13. How many grams of Ca(OH)2 are required to react with 2.36 mol of H3PO4 to prod Ca3(PO4)2 according to the equation ? 3Ca(OH)2 + 2H3PO4 +Ca3(PO4)2 + 6H2O
Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 30.00 mL of 0.00150 M calcium hydroxide. _____ Ca(OH)2(aq) + _____ H3PO4(aq) → _____ Ca3(PO4)2(aq) + _____ H2O(l) 15.0 mL 2.02 mL 10.0 mL 22.5 mL
You titrate 41.27 mL of 0.108 M Ca(OH)2 into 25.00 mL of citric acid (C6H307) (triprotic). What is the balanced equation and the molarity of the acid? Select both an equation and a molarity. CH3O+ (aq) + Ca(OH)2 (aq) - H20 (1) + Ca3(C6H507)2 (aq) 2C6H307 (aq) + 3Ca(OH)2 (aq) + 6H20 (1) + Ca3(C6H507)2 (aq) CH807 (aq) + Ca(OH)2 (aq) - H20 (1) + CaC6H507 (aq) 3C6H307 (aq) + 2 Ca(OH)2 (aq) + 6H20 (1) + Ca3(C6H507)2 (aq) 0.267...
14.93 mL of an unknown-concentration NaOH solution is used to fully titrate 3.00 g of a benzoic acid primary standard. What is the concentration of the NaOH solution? Answer is in molarity (M), rounded to 3 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...
Homework Acids and Bases Name: 1) Write in the products for this acid-base neutralization reaction, then balance the equation. HBr(aq) + Ca(OH)2(aq) → 2) A 8.00-ml sample of an H.PO, solution of unknown concentration is titrated with a 0.2090 M NaOH solution. A volume of 6.12 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4 solution? 3 NaOH + H3PO4 → Na3PO4 + 3 H20 3) What volume in...
If it takes 32 mL of 0.1M NaOH to fully titrate 20mL of an unknown monoprotic acid, what was the initial concentration of an unknown acid before titration.
35.25 mL of NaOH solution are required to titrate 0.5745 g of an unknown monoprotic acid. Prior standardization of the NaOH determined its concentration as 0.1039 M. 1. Use the data provided to determine the molar mass of the unknown acid 2. If 20 mL of a 1.0 M solution of the unknown monoprotic acid is placed into a beaker and 10 mL of 0.1 M NaOH is added, the pH of the final solution is 1.9. What is the...
A 0.205 M NaOH solution is used to titrate 20.0 mL of solution of H2SO4. Write a balanced equation for this acid base reaction If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4solution. What is the PH of the solution if the hydroxide concentration [OH-] is 4.3 x 10-6M.
Q2. A. Calculate the volume in ml of a 1.72 M Ca(OH), solution required to react with a 250 ml of a 1.8 M H3PO4 solution in anacid-base reaction. (use short-cut technique without balancing) H3PO4(aq) + Ca(OH)2(aq)Ca3(PO.). (aet) + H20 unbalanced B.Calculate the volume of solution required to prepare 2.0 MCa3(PO4)2 by dissolving 62 grams Ca3(PO4)2 in water. Ca=40 0=16 P=31 C. In dilution, what volume of 4.0 M HNO3 (aq) stock (initial) solution is required to prepare a 3.0...