A Titration used 24.5mL of 0.10M KOH to neutraliz an acid. How many moles of KOH were required for the neutralization?
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A Titration used 24.5mL of 0.10M KOH to neutraliz an acid. How many moles of KOH...
How many moles of acetic acid could be in the 25% acetic acid solution before the extraction occurs? 100% acetic acid has 0.0394 moles present. 0.00985 moles 0.985 moles 0.158 moles Calculate how many moles of acetic acid were present in the aqueous layer after the extraction of 5% acetic acid. Use the data from the titration below to calculate your answer. Titration data: 0.1000M NaOH, 1.45 mL used to reach end point of titration. Group of answer choices 0.000795...
3. Consider the following neutralization reaction: HI+KOH → H2O +KI a) How many moles of HI are in a 100 ml solution with a pH of 1.22? b) How many moles of KOH are in 20 mL of a 0.15 M solution? c) If the solutions from A and B are mixed, how many moles of HI are remaining? d) What would be the pH of the resulting solution?
Calculate how many moles of acetic acid were present in the aqueous layer after the extraction of 5% acetic acid. Use the data from the titration below to calculate your answer. Titration data: 0.1000M NaOH, 1.45 mL used to reach end point of titration. Group of answer choices 0.000795 moles 0.725 moles 0.000145 moles
If 17.06 mL of acetic acid are used in a titration and the molarity of the acetic acid is 0.12, how many moles of acetic acid are used?
In an acid-base titration, the neutralization of 20.00 mL of a solution of KOH (potassium hydroxide) of unknown concentration required the addition of 28.60 mL of 0.1042 M HNO3 (nitric acid). Calculate the molarity of the potassium hydroxide solution. Place your answer in the box. Express your answer using only a number or numbers without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.
In a titration, 23.57 mL of 1.37 M NaOH were added to an acid. How many moles of NaOH were added? Enter a numerical value in the correct number of significant figures. Do not enter units and do not use scientific notation. In a titration, 50.00 mL of 0.916 M H2SO4 were added. How many moles of H* were delivered? Enter a numerical value in the correct number of significant figures. Do not enter units and do not use scientific...
Fall 10.PUI How many moles of base were required to react completely with the acid in this reaction? mol Ca(OH)2 Part 2 (0.7 point) See Hint How many moles of HCl were present in the original 25.00 mL of acid? mol HCI Part 3 (0.7 point) What is the molarity of the original HCl solution? Choose one: O 0.0716 M O 0.179 M O 0.286 M O 1.79x10-4 M O 0.424 M Ca(OH)2(aq) + 2HCl(aq) — CaCl, (aq) +H20(1) An...
15 In an acid-base titration, the neutralization of 25.00 mL of a solution of KOH (potassium hydroxide) of unknown concentration required the addition of 22.60 mL of 0.1532 M HNO3 (nitric acid). Calculate the molarity of the potassium hydroxide solution Place your answer in the box. Express your answer using only a number or numbers without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured,
What is a polyprotic acid? 2. How many moles of H3O + are present in 50 mL of 0.3 M H2SO4? 4. If 20.20 mL of 0.122 M NaOH are required to reach the first equivalence point of a solution of citric acid (H3C6H5O7), how many mL of NaOH are required to completely neutralize this solution? 5. If the pH at one-half of the neutralization points of a dibasic acid is 3.52 and 6.31 respectively, what are the values for...
To calculate the concentration of a solution using acid–base titration data. In an acid–base titration, an acid (or base) of known concentration is added to a base (or acid) of unknown concentration until the number of moles of H+ and OH- are equal, a condition called the equivalence point. Since you know the number of moles of H+ (or OH- ) that you added, you can determine the number of moles of OH- (or H+) in the unknown solution. For...