# A solution of 0.25 M NaOH is used to neutralize 25.0 mL of H3PO4 solution. If 33.0 mL of NaOH is...

## Question:

A solution of 0.25 M {eq}NaOH {/eq} is used to neutralize 25.0 mL of {eq}H_3PO_4 {/eq} solution. If 33.0 mL of {eq}NaOH {/eq} is required to reach the endpoint, what is the molarity of the {eq}H_3PO_4 {/eq}?

a) 0.042 M

b) 0.50 M

c) 3.78 M

d) 1.26 M

e) 0.11 M

## Molarity:

In describing solution concentrations, molarity (M) refers to the amount of solute present in a liter of solution. In addition to this, the molar concentration is usually expressed in moles per liter; however, several units can still be used as long as it agrees with mol/L when the dimensional analysis is used.

## Answer and Explanation: 1

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

View this answer

The reaction between {eq}NaOH{/eq} and {eq}H_3PO_4{/eq} is written below where 3 moles of {eq}NaOH{/eq} are required to neutralize 1 mole of...

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 8 / Lesson 4What is molarity? What is molality? Compare molarity vs molality by viewing molality and molarity formulas, how to calculate molarity and molality, and examples.

#### Related to this Question

- 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 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?
- 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?
- 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?
- 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.
- 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 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?
- 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 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.
- 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
- 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)?
- 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?
- 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 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?
- What volume of a 0.150 M NaOH solution is required to completely neutralize 50.0 mL of a 0.150 M H3PO4 solution?
- 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?
- 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?
- 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 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 H3PO4 solution?
- How many mL of a 0.10 M NaOH solution are needed to neutralize 15 mL of 0.20 M H3PO4?
- 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 (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 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.
- 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.
- 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?
- How many milliliters of 0.150 M NaOH are required to completely neutralize 7.00 mL of 0.300 M H3PO4?
- How many milliliters of 0.105 M NaOH are required to neutralize exactly 14.2 mL of 0.141 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 mL of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO4?
- 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 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?
- 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 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
- 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
- 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
- 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 milliliters) of 0.171 M H3PO4 required to neutralize 36.2 mL of 0.259 M NaOH solution.
- How many milliliters of 0.100 M NaOH is needed to completely neutralize 25.0 mL of 0.250 M H3PO4?
- How many mL of 0.175 M H3PO4 are needed to neutralize 15.00 mL of 0.33 M NaOH?
- 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?
- 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 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
- 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:
- How many mL of 0.500 M NaOH would neutralize 25.00 mL of 0.100 M H3PO4?
- What is the number of moles of NaOH required to titrate 38.05 mL of a 1.500 M H3PO4 solution?
- How much H_3PO_4, in moles, is needed to neutralize 1 L of a 0.75 M solution of NaOH?
- 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?
- 27. The titration of 80.0 mL of an unknown concentration H_3PO_4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H_3PO_4 solution? a. 1.03 M b. 0.343 M c. 0.114 M
- How many mL of 0.48 M NaOH are needed to neutralize 2.00 moles of 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) 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
- If 29.8 ml of the H_3PO_4 (phosphoric acid) reacts with 35.0 mL of 5.00 M KOH, what is the molarity of the acid? H_3PO_4 + 3KOH \rightleftharpoons K_3PO_4 + 3H_2O
- 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.
- 20 ml of 0.15 M H_3PO_4 is required to neutralize 40 ml of a KOH solution. The molarity of the KOH solution is ________. H_3PO_4 + 3 KOH longrightarrow K_3PO_4 + 3 H_2O
- 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
- If 86 ml of 1.2 m Ba(OH)2 and 20 ml of H3PO4 are mixed together, what molarity of the acid is needed to neutralize the base?
- A solution of 0.168 M NaOH is used to neutralize 21.5 mL of a H2SO4 solution. If 30.0 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4 solution?
- A 5.00 mL sample of an aqueous solution of H_3PO_4 requires 43.2 mL of 0.285 M NaOH to convert all of the H_3PO_4 to Na_2HPO_4. The other product of the reaction is water. Calculate the molarity of th
- In the titration of 100 mL of a 0.1 M H_3PO_4 with 0.5 M NaOH, calculate the pH of the solution at each of the following points: a) before any NaOH added b) after 10 mL of NaOH added c) at first equiv
- Suppose 25.0 mL of a solution containing 0.100 M H3PO4 is titrated with 0.200 M NaOH. Calculate the pH of the solution after 10.0 mL of NaOH is added.
- Suppose 25.0 mL of a solution containing 0.100 M H3PO4 is titrated with 0.200 M NaOH. Calculate the pH of the solution after 20.0 mL of NaOH has been added.
- A 30.0 mL sample of phosphoric acid is titrated with 18.0 mL of 3.0 M NaOH solution. What is the molarity of the phosphoric acid?
- Suppose 25.0 mL of a solution containing 0.100 M H3PO4 is titrated with 0.200 M NaOH. How much NaOH is needed to reach the second equivalence point? Calculate the pH of the solution at that point.
- 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
- 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
- A solution contains 10.0 m mol of H_3PO_4 and 5.0 mmol of NaH_2PO_4. How many millimeters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H_3PO_4 with NaOH?
- Suppose 25.0 mL of a solution containing 0.100 M H3PO4 is titrated with 0.200 M NaOH. How many mL of NaOH are needed to reach the first equivalence point? Calculate the pH of the solution at that point.
- 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 solution contains 10. mmol of H3PO4 and 5.0 mmol of NaH2PO4. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?
- 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
- A solution of 0.162 M NaOH is used to titrate 23.5 mL of a solution of H2SO4. If 37.0 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H2SO4 solution?
- Calculate the molarity of an HBr solution if 23.47 mL of solution is required to neutralize 29.09 mL of 0.1010 M NaOH.
- Calculate the molarity of a phosphoric acid solution if 34.21 mL of a 0.043 M sodium hydroxide solution neutralizes 25.00 mL of the acid solution.
- How many mL of 0.500 M NaOH are necessary to neutralize 20.0 mL of each of the following acids? a) 0.150 M HNO3 b) 0.250 M H2SO4 c) 0.450 M H3PO4
- 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_
- A 0.100 g sample of phosphoric acid (MW = 99.0 g/mol), a tri-protic acid, requires 35.0 mL of a NaOH solution for neutralization. What is the molarity of the NaOH solution?
- Suppose 25.0 mL of a solution containing 0.100 M H3PO4 is titrated with 0.200 M NaOH. Calculate the pH of the solution before any NaOH is added.
- 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?
- What is the molarity of a NaOH solution if 48.0 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?
- What is the molarity of a NaOH solution if 28.2 mL of 0.112 M H_2SO_4 solution is required to neutralize a 25.0 mL sample of NaOH solution? (a) 0.199 (b) 39.5 (c) 0.253 (d) 0.0993 (e) 0.126
- Calculate the pH during the titration of 50.00 mL of 0.1000 M phosphoric (H_3PO_4; Ka_1 = 7.1 times 10^{-3}, Ka_2 = 6.3 times 10^{-8}, Ka_3 = 2 times 10^{-13}) after adding 21.05 mL of 0.1000 M NaOH.
- 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?
- 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?
- What volume of 0.20 M H3PO4 is needed to react with 100 mL of 0.1 M NaOH?
- What volume of a 1.25 M NaOH solution is required to neutralize 13.3 mL of a 0.139 M phosphoric acid solution?
- A solution contains 25 mmol of H_3PO_4 and 10 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_3PO4 with NaOH?
- If 42.00 mL of a 0.1274 M NaOH solution is required to neutralize 13.02 mL of an H2SO4 solution, what is the molarity of the acid solution?
- If 11.43 mL of a 0.1203 M NaOH solution is required to neutralize 34.59 mL of an H2SO4 solution, what is the molarity of the acid solution?