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

## Question:

What volume in mL of a 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}?

Determine if each of the following substances is acidic, basic, or neutral. Also, calculate the {eq}H_3O^+ {/eq} and {eq}OH^- {/eq} concentration of the solutions.

## End Point:

At the end point of the reaction, the reaction undergoes completion and the amount of the both the substance, that are acid and base becomes equal. The following equation is used to determine the concentration or volume of any substance required to reach the end point of the reaction:

{eq}\rm M_1V_1 = M_2 V_2 {/eq}

Here, 1 and 2 indicate the solutions

M and V indicate the molarity and volume respectively.

## Answer and Explanation: 1

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

View this answerWe are given:

- Molarity of NaOH = {eq}\rm 0.0992\ M {/eq}

- Molarity of {eq}\rm H_3PO_4 = 0.107\ M {/eq}

- Volume of {eq}\rm H_3PO_4 = 15.0\ mL {/eq}

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 13 / Lesson 4Discover what the formula for an endpoint is. Answer the question, "Does a line have an endpoint?" Read about endpoints and midpoints. Use the endpoint equation.

#### Related to this Question

- What volume (in mL) of 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 H3PO4?
- 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.
- 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 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.
- 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 33.55 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 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?
- 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?
- 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?
- 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?
- 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
- 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 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 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 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 H3PO4, 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 H_3PO_4, how many mL of 0.2625 M NaOH are needed to reach the point of complete neutralization?
- 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.
- 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)?
- In the lab, you set up a titration experiment with 30.0 mL of 0.100 M H3PO4 solution in a flask and 0.120 M NaOH in the buret. Determine the volume (in mL) of NaOH solution needed to neutralize the acid. (Hint: Write and balance the equation for neutraliz
- 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?
- 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 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?
- 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
- 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 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?
- 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?
- 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?
- 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?
- 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 33.00 mL sample of an unknown H3PO4 solution is titrated with a 0.110 M NaOH solution. The equivalence point is reached when 26.03 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is H3P
- 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
- 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?
- Calculate the volume (in milliliters) of 0.171 M H3PO4 required to neutralize 36.2 mL of 0.259 M NaOH solution.
- 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 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
- 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?
- 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?
- Calculate the volume of 0.730 M NaOH solution needed to completely neutralize 58.9 mL of a 0.700 M solution of the monoprotic acid HBr. __________ mL NaOH
- 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?
- 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?
- 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?
- 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 0.20 M H3PO4 solution?
- A) A 5.10 mL sample of an H_3PO_4 solution of unknown concentration is titrated with a 9.300 \times 10^{-2} M NaOH solution. A volume of 7.22 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H_3
- 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?
- Calculate the volume, in milliliters, of a 0.200 M NaOH solution that will completely neutralize each of the following: - 3.9 mL of a 1.22 M HNO3 solution. - 8.2 mL of a 0.845 M 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?
- 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?
- 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 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?
- How many mL of a 0.10 M NaOH solution are needed to neutralize 15 mL of 0.20 M H3PO4?
- In a acid-base titration, 22.81 mL of an NaOH solution were required to neutralize 26.18 mL of a 0.1121 M HCl solution. What is the molarity of the NaOH solution?
- 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
- 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 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_
- Calculate the volume of 0.850-M NaOH solution needed to completely neutralize 25.8 mL of a 0.370-M solution of the monoprotic acid HCl.
- What volume of a 1.25 M NaOH solution is required to neutralize 13.3 mL of a 0.139 M phosphoric acid solution?
- In an acid-base titration, 22.13 mL of a NaOH solution is needed to neutralize 24.65 mL of a 0.1094 M HCl solution. What is the molarity of the NaOH solution?
- 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?
- 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?
- 1.12 g of KHP required 34.38 mL of an approximately 0.3 m NaOH solution in an acid/base titration to reach the equivalence point. What is the exact molarity of the NaOH 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.
- 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
- 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.
- 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.
- 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?
- 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 0.100 M NaOH are required to neutralize (or titrate) 25.0 mL of 0.15 M H_3PO_4?
- 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?
- 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.
- 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?
- Calculate the volume of 0.340-M NaOH solution needed to completely neutralize 88.6 mL of a 0.870-M solution of the monoprotic acid HBr.
- Calculate the volume of a 0.810 M NaOH solution needed to completely neutralize 10.9 mL of a 0.840 M solution of the monoprotic acid HBr.
- 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))?
- A 34.00 mL sample of an unknown H3PO4 solution is titrated with a 0.130 M NaOH solution. The equivalence point is reached when 26.98 mL of NaOH solution is added. What is the concentration of the unk
- 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?
- What volume (in mL) of 0.812 M HCl solution is required to titrate 1.45 g of NaOH to the equivalence point?
- Calculate the volume (in mL) of a 6.0 M NaOH solution that would be necessary to prepare 2.0 L of a 0.1 M NaOH solution.
- Acid-base titration SOLVE ALL 5 questions. 1. If 20.00 mL of 0.2019 M HCI requires 39.63 mL of a NaOH solution for complete neutralization, what is n the answer? 2. How many milliliters of 14.5 M NH
- In a titration, 25.0 mL of KHP is titrated to the equivalence point with NaOH. The final solution volume is 45.5 mL. What was the volume of NaOH used in the titration? (a) 25.0 mL. (b) 20.5 mL. (c) 70
- 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?
- What is the number of moles of NaOH required to titrate 38.05 mL of a 1.500 M H3PO4 solution?
- How many mL of 0.300 M NaOH (base) solution are required to neutralize 15.0 mL of 0.250 M HCl (acid) solution?
- If 10.0 mL of 0.100 M HCl is titrated with 0.200 M NaOH, what volume of sodium hydroxide solution is required to neutralize the acid?
- A solution contains 25 mmol of H_3PO_4 and 10.0 mmol of NaH_2PO_4. What volume of 2.0 M NaOH must be added to reach the second equivalence point of the titration of the H_3PO_4 with NaOH? A) 5.0 mL B) 60.0 mL C) 12 mL D) 30.0 mL E) 25 mL
- A) 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 u
- 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).
- A 21.34 mL sample of 0.1732 M HCl solution requires 28.92 mL of NaOH solution for complete neutralization. a. Calculate the number of moles of NaOH required to completely neutralize the NaOH. b. Calculate the molarity of the NaOH solution.
- 1. A sample of weak acid was titrated against NaOH, and it required 14.53 mL to be fully neutralized. Calculate the volume of NaOH required to reach 60% neutralization. 2. Another aliquot of the sam
- A 25.00 mL sample of HCl is titrated with a 0.315 M NaOH solution. If 22.65 mL of the NaOH solution is required to titrate the acid, what is the molarity of the HCl solution?
- How many milliliters of 0.100 M NaOH is needed to completely neutralize 25.0 mL of 0.250 M H3PO4?