# What volume (in mL) of 0.0992 M NaOH solution is required to reach the endpoint in the complete...

## Question:

What volume (in mL) of 0.0992 M {eq}NaOH {/eq} solution is required to reach the endpoint in the complete titration of a 15.0 mL sample of 0.107 M {eq}H_3PO_4 {/eq}?

## Equivalence Point:

An acid-base titration experiment seeks to determine the unknown molarity of some acidic/basic analyte reactant. It is titrated with a basic/acidic titrant reactant of known molarity. The reaction continues until you have combined the reactants in stoichiometric quantities. This is the equivalence point of the titration and here there is no limiting reactant. The data here is used to determine the analyte moles, which leads to the analyte molarity. The equivalence point is often referred to as the endpoint, according to the change in color of some indicator chemical at some pH value. The pH value is commonly assumed to be the actual equivalence point pH.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerNaOH is a strong monoprotic base. Phosphoric acid is a weak triprotic acid. The balanced reaction equation is:

{eq}\rm 3NaOH + H_3PO_4 \rightarrow...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 12 / Lesson 11Learn about equivalence point and end point in titrations. Examine how to find equivalence points in a variety of ways, and discover the steps to do so.

#### Related to this Question

- What volume in ml of 0.0985 M NaOH solution is required to reach the end point in the complete titration of a 15.0 ml sample of 0.124 M phosphoric acid?
- What volume in mL of a 0.0992 M NaOH solution is required to reach the endpoint in the complete titration of a 15.0 mL sample of 0.107 M H_3PO_4? Determine if each of the following substances is acidic, basic, or neutral. Also, calculate the H_3O^+ and OH
- A 25.0 mL sample of H3PO4 is titrated with NaOH. If 29.2 mL of 0.738 M NaOH is needed to reach the endpoint, what is the concentration (M) of the H3PO4 solution?
- Calculate the volume (in mL) of a 1.350 M NaOH solution required to titrate 25.0 mL of a 1.500 M H3PO4 solution.
- Calculate the volume (in mL) of a 1.420 M NaOH solution required to titrate 25.00 mL of a 1.500 M H3PO4 solution.
- Calculate the volume (in mL) of a 1.450 M NaOH solution required to titrate 25.00 mL of a 1.800 M H3PO4 solution.
- If a solution of 0.105 M NaOH is used to titrate 50.0 mL of a 0.0224 M H_3PO_4 solution, what volume of NaOH solution in mL is required?
- If a solution of 0.105 M NaOH is used to titrate 50.0 mL of a 0.0224 M H3PO4 solution, what volume of NaOH solution in mL is required?
- A solution of 0.190 M NaOH is used to titrate 53.5 mL of a 0.0324 M H_3PO_4 solution. What volume, in milliliters, of the NaOH solution is required? H_3PO_4(aq)+3NaOH(aq)\to 3H_2O(l)+Na_3PO_4(aq)
- A solution of 0.24 M NaOH is used to titrate 50.0 mL of a 0.0224 M H_3PO_4 solution. What volume, in milliliters, of the NaOH solution is required? H_3PO_2(aq) + 3NaOH(aq) rightarrow 3H_2O(l) + Na_3PO
- Calculate the volume of a 1.420 M NaOH solution required to titrate 33.55 mL of a 1.500 M H_3PO_4 solution.
- Calculate the volume of a 1.420 M NaOH solution required to titrate 31.95 mL of a 1.500 M H3PO4 solution.
- Calculate the volume of a 1.420 M NaOH solution required to titrate 25.00 mL of a 1.500 M H_3PO_4 solution.
- Calculate the volume of a 1.420 M NaOH solution required to titrate 30.80 mL of a 1.500 M H_3PO_4 solution.
- A 5.00-mL sample of an H3PO4 solution of unknown concentration is titrated with a 0.1003 M NaOH solution. A volume of 6.55 mL of the NaOH solution was required to reach the endpoint. What is the conce
- A solution of 0.25 M NaOH is used to neutralize 25.0 mL of H3PO4 solution. If 33.0 mL of NaOH is required to reach the endpoint, what is the molarity of the H3PO4? a) 0.042 M b) 0.50 M c) 3.78 M d) 1.26 M e) 0.11 M
- A 100.0 ml sample of 0.50 M HCl (aq) is titrated with a 0.10 M NaOH. What volume of the NaOH solution is required to reach the endpoint of the titration?
- If you have 10.00 mL of 0.5875 M H_3PO_4, how many mL of 0.2625 M NaOH are needed to reach the point of complete neutralization?
- If you have 10.00 mL of 0.5875 M H3PO4, how many mL of 0.2625 M NaOH are needed to reach the point of complete neutralization?
- What is the molarity of an unknown H_3PO_4 acid if 10.00 mL of it was titrated with 0.103 M NaOH and 54mL of NaOH was required to reach the endpoint of the titration?
- A 25.0 mL sample of H3PO4 requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid?
- What volume of a 0.150 M NaOH solution is required to completely neutralize 50.0 mL of a 0.150 M H3PO4 solution?
- A triprotic acid, H3PO4, required 42.50 mL of 0.50 M NaOH to reach the endpoint. Calculate the concentration of the acid if 27.55 mL of the acid was used in the titration.
- What volume (in mL) of 0.0985 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 15.0-mL sample of 0.124 M phosphoric acid?
- What volume in mL of 0.0985 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 15 mL sample of 0.124 M phosphoric acid?
- What volume in milliliters of 9.750x10-2 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 14.0 mL sample of 0.144 M phosphoric acid?
- What volume in mL of a 0.121 M NaOH solution is required to reach the equivalence point in the complete titration of a 15.0 mL sample of 0.112 M H2SO4?
- What volume of a 0.100 M solution of NaOH is needed to completely neutralize 50.0 mL of a 0.100 M H3PO4 solution?
- What volume in milliliters of a 0.101 M NaOH solution is required to reach the equivalence point in the complete titration of a 15.0 mL sample of 0.122 M H_2SO_4?
- What is the molarity of a NaOH solution if 21.3 mL of the NaOH solution is neutralized by 10.4 mL of 6.10 M H_3PO_4?
- How many mL of a 0.10 M NaOH solution are needed to neutralize 15 mL of 0.20 M H3PO4 solution?
- How many mL of a 0.10 M NaOH solution are needed to neutralize 15 mL of a 0.20 M H_3PO_4 solution?
- How many mL of a 0.10 M NaOH solution are needed to neutralize 15 mL of a 0.20 M H3PO4 solution?
- How many mL of a 0.10 M NaOH solution is needed to neutralize 15 mL of 0.20 M H3PO4 solution?
- In a titration of 35 mL of 0.40 M H_3PO_4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has
- Calculate the volume, in mL, of a 0.216 M NaOH solution that will completely neutralize 8.60 mL of a 0.825 M H3PO4 solution.
- How many mL of a 0.10 M NaOH solution are needed to neutralize 15 mL of 0.20 M H3PO4?
- If 23.6 ml of 0.200 m NaOH is required to neutralize 10.00 ml of a H_3PO_4 solution , what is the concentration of the phosphoric acid solution?
- If 38.19 mL of 0.084 M NaOH was dispensed to get to the endpoint of a titration of 25 mL of H3PO4, what was the initial concentration of H3PO4?
- What is the molar concentration of 799.0 mL of an aqueous H3PO4 solution that required 0.02947 L of an 837 mM standard solution of NaOH for complete neutralization?
- A 14.3-mL sample of an H3PO4 solution is titrated with a 1.16 M NaOH solution. The neutralization reaction is complete when 34.6 mL of NaOH is added. What is the concentration of the H3PO4 solution (in M)?
- What volume in milliliters of 9.950 x 10^(-2) M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 17.0 mL sample of 0.144M phosphoric acid?
- What is the molarity of a solution of H_3PO_4 if 11.1 mL is neutralized by 33.2 mL of 0.161 M NaOH?
- A 22.9 mL sample of H3PO4 (triprotic) solution is titrated with a 0.405 M NaOH solution. The equivalent point is reached when 44.1 mL of NaOH solution is added. What is the concentration of the H3PO4 solution?
- A 29.30 mL sample of an H3PO4 (triprotic) solution is titrated with a 0.48 M NaOH solution. The equivalence point is reached when 45.70 mL of NaOH solution is added. What is the concentration of the H3PO4 solution?
- A solution of 0.330 M KOH is used to neutralize 17.0 mL of a 0.188 M H3PO4 solution. What volume, on milliliters, of the KOH solution is required to reach the endpoint? H3PO4(aq) + 3KOH(aq) → 3H2O(l) + K3PO4(aq)
- A 30.1 mL sample of H_3PO_4 solution is titrated with a 0.609 M NaOH solution. The equivalence point is reached when 50.1 mL of NaOH solution is added. What is the concentration H_3PO_4 solution?
- A 29.30 mL sample of an H3PO4 solution is titrated with a 0.48 M NaOH solution. The equivalence point is reached when 45.70 mL of NaOH solution is added. What is the concentration of the H3PO4 solution?
- What is the number of moles of NaOH required to titrate 38.05 mL of a 1.500 M H3PO4 solution?
- Calculate the volume (in milliliters) of 0.171 M H3PO4 required to neutralize 36.2 mL of 0.259 M NaOH solution.
- How many milliliters of 0.105 M NaOH are required to neutralize exactly 14.2 mL of 0.141 M H3PO4?
- How many milliliters of 0.150 M NaOH are required to completely neutralize 7.00 mL of 0.300 M H3PO4?
- A titration involves titrating 0.4 M NaOH into a solution of 0.2 M H3PO4. a. Calculate the volume of NaOH that will be required to reach the first equivalence point. b. Calculate the volume of NaOH re
- Using 0.1M solution of NaOH, 25 mL 0.4823M HCl solution was required to titrate to the end point. What is the volume of 0.1M solution of NaOH to be used?
- What volume of 0.115 M NaOH is required to reach the equivalence point in the titration of 25.00 mL of 0.200 M of HF? Ka(HF) = 7.4 times 10^(-4).
- What volume of 0.750 M NaOH solution would be required to neutralize completely 100 mL of 0.250 M H_3PO_4 solution? 3NaOH + H_3PO_4 \longrightarrow Na_3PO_4 + 3H_2O
- How many mL of 0.100 M NaOH are required to neutralize (or titrate) 25.0 mL of 0.15 M H_3PO_4?
- How many mL of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO4?
- How many mL of 0.01 M NaOH will be required to titrate 0.061 g of KHP to it's endpoint?
- How many ml of 0.01-m NaOH will be required to titrate 0.062-g of KHP to its endpoint?
- If 44.9 ml of 0.179 M hydrochloric acid requires 21.2 ml of the NaOH solution to reach the endpoint, what is the molarity of the NaOH solution?
- Using a 0.1M solution of NaOH, 25 mL 0.4823 M HCl solution was required to titrate to the end point. What is the volume of 0.1 M solution of NaOH to be used?
- What volume of a 1.25 M NaOH solution is required to neutralize 13.3 mL of a 0.139 M phosphoric acid solution?
- Calculate the volume of 0.07731 M NaOH needed to titrate: a) 25.00 mL of a solution that is 0.03000 M in HCl and 0.01000 M in H_3PO_4 to a bromocresol green end point. b) the solution in a) to a thymolphthalein end point. c) 30.00 mL of 0.06407 M NaH_2PO_
- How many milliliters of 0.100 M NaOH is needed to completely neutralize 25.0 mL of 0.250 M H3PO4?
- If your titration solution is 0.425 M in NaOH, and the endpoint occurs at 13.40 mL of titrant, how many mmol of NaOH are required to reach the endpoint?
- If your titration solution is 0.406 M in NaOH, and the endpoint occurs at 13.10 mL of titrant, how many mmol of NaOH are required to reach the endpoint?
- The titration of a 25.00 mL sample of NaOH required 28.25 mL of a 0.200 M HCl solution to reach the endpoint. What was the molar concentration of the sodium hydroxide solution?
- What volume of 0.1500 M NaOH is required to titrate 22.00 mL of 0.1250 M HCl? (Answer in mL)
- What volume of a 0.68 M HCl solution is required to titrate 27.2 mL of a 0.539 M NaOH solution?
- How many mL of 0.175 M H3PO4 are needed to neutralize 15.00 mL of 0.33 M NaOH?
- 1) What volume of 0.1M H2SO4 solution is needed to neutralize 40 mL of 0.2M NaOH solution? 2) If 25 mL of 0.2 M H3PO4 solution is needed to neutrailize 60 mL of Ba(OH)2, then what is the molarity of
- A 12 mL sample of vinegar(aq), CH_3COOH, requires 24.5 mL of 0.400 M NaOH to reach the endpoint in a titration. What is the molarity of the acetic acid solution?
- What volume of 0.1084 M sodium hydroxide (NaOH (aq)) would be required for complete neutralization of 270 mL of 0.1084 M phosphoric acid (H_3PO_4 (aq))?
- What volume (in mL) of 0.812 M HCl solution is required to titrate 1.45 g of NaOH to the equivalence point?
- What volume of 0.1500 M NaOH is required to titrate 20.00 mL of 0.1000 M HCI?
- A solution of 0.3044 M KOH is used to neutralize 16.00 mL of an H3PO4 solution. If 28.48 mL of the KOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution?
- Calculate the volume (in mL) of a 1.350 M NaOH solution required to titrate 25.0 mL of a 2.450 M HCI solution.
- If 33.0 mL of 0.002 M aqueous H_3PO_4 is required to neutralize 28.0 mL of an aqueous solution of NaOH, determine the molarity of the NaOH solution.
- A 5.20 mL sample of a H_3PO_4 solution of unknown concentration is titrated with a 9.800 times 10^{-2} M NaOH solution. A volume of 7.12 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H_3PO_4
- The cola sample is 50.0 mL, the equivalence point volume is 13.4 mL, and the NaOH solution concentration is 0.025 M, what mass of H_3PO_4 was in the sample?
- If 24.5 mL of the 0.10 M NaOH solution is required to reach the endpoint in a titration with an unknown monoprotic acid, how many moles of the acid were present?
- What is the volume (mL) of 5 M NaOH solution required to dilute it to final volume of 575 mL and at final concentration?
- How many millilitres of 0.100 M NaOH are needed to completely neutralize 25.0 mL of 0.250 M H_3PO_4? A. 62.5 mL B. 125 mL C. 31.3 mL D. 188 mL E. 78.1 mL.
- What volume of 0.1700 M NaOH is required to titrate 22.00 mL of 0.1100 M HCl?
- What volume of 0.1600 M NaOH is required to titrate 22.00 mL of 0.1100 M HCl?
- A 35.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.28 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution?
- A 22.0-mL sample of an unknown H3PO4 solution is titrated with a 0.110 M NaOH solution. The equivalence point is reached when 18.60 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution?
- A 25.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.33 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution?
- Calculate the volume (in mL) of a 1.450 M NaOH solution required to titrate 25.00 mL of a 2.450 M HCl solution.
- Calculate the volume (in mL) of a 1.420 M NaOH solution required to titrate 25.00 mL of a 2.430 M HCl solution.
- What volume of 0.20 M H3PO4 is needed to react with 100 mL of 0.1 M NaOH?
- How many milliliters of 0.150 M NaOH solution are required to titrate 40.0 mL of a 0.100 M HNO_{2} solution?
- How many milliliters of a 0.610 M NaOH solution are needed to completely neutralize 25.0 mL of a 0.356 M phosphoric acid solution?
- A titration required 23.8 mL of a 0.15 M NaOH solution. How many moles of NaOH were in this volume?
- What volume in milliliters of 9.750 times 10^2 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 17.0 mL sample of 0.124 M phosphoric acid? Express the answer using three significant figures.
- Consider the titration of 10.0 mL of a 0.200 M HF solution with a 0.0998 M NaOH solution. What volume of the NaOH solution is required to reach the equivalence point?
- 3 mL of 0.15 M solution of NaOH was added in 10 mL of 0.05 M solution of H3PO4. Calculate the concentration of HPO42- ions.(pKas of phosphoric acid = 2.15; 7.2; 12.3).The 3 mL of 0.15 M solution of NaOH was added in 10 mL of 0.05 Msolution of H3PO4. Calcu
- A 27.00 ml sample of an unknown H_3PO_4 solution is titrated with a 0.110 M NaOH solution. The equivalence point is reached when 25.78 ml of NaOH solution is added. What is the concentration of the unknown H_3PO_4 solution? The neutralization reaction is:
- A 30.00 mL sample of an unknown H_3PO_4 solution is titrated with a 0.120 M NaOH solution. The equivalence point is reached when 25.23 mL of NaOH solution is added. What is the concentration of the unknown H_3PO_4 solution? The neutralization reaction is