What volume of 0.125 M oxalic acid, H₂C₂O4, is required to react with 95.5 mL of 0.717 M NaOH? H₂C₂O4 (aq) + 2 NaOH(aq) → Na2 C₂O4 (aq) + 2 H₂O(l) Volume = Submit Answer L Try Another Version [References] 4 item attempts remaining

What volume of 0.125 M oxalic acid, H₂C₂O4, is required to react with 95.5 mL of 0.717 M NaOH? H₂C₂O4 (aq) + 2 NaOH(aq) → Na2 C₂O4 (aq) + 2 H₂O(l) Volume = Submit Answer L Try Another Version [References] 4 item attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: How many milliliters of 0.237 M Ca(OH)2 are needed to react with 0.00356 moles of Cl2 in the…

Q: 1) What volume of 0.109 M HNO3 is required to react completely with 2.500 g Ba(OH)2? Express your…

A: The given reaction is balanced as follows, It is clear that about 2 moles of HNO3 is required to…

Q: Zinc reacts with hydrochloric acid according to the reaction equation Zn(s) + 2 HCl(aq) → ZnCl₂(aq)…

Q: For the following reaction, how many grams of Pb(Br)2 will formed from 150.0 mL of a 0.150 M KBr…

Q: How many grams of AgCI will be formed when 60 mL of 0.500M AGNO, is completely reacted according to…

A: The balanced reaction taking place is given as, Given : Concentration of AgNO3 = 0.500 M And volume…

Q: Determine the volume of 0.215 MM KOHKOH solution required to neutralize each sample of sulfuric…

A: To find: The volume required to neutralize the given solution

Q: I2 (aq) + 2 Na2S2O3 (aq) → 2 NaI (aq) + Na2S4O6 (aq) It takes 62.25 ml of…

A: The concentration of Na2S2O3 solution is 0.0400 M.The volume of Na2S2O3 solution is 62.25 mL.The…

Q: he following reaction takes place as represented by the balanced chemical equation below: Mg(NO3)2…

A: The given balanced equation is- Mg(NO3)2 (aq) + 2 NaOH (aq) → Mg(OH)2 (s) + 2 NaNO3 (aq) As…

Q: Consider the following balanced chemical reaction: H2SO4 (aq) + 2 KOH (aq) ------------> K2SO4…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: * 00 F Strontium chloride and sodium fluoride react to form strontium fluoride and sodium chloride…

Q: Using the information in the table below, identify the limiting reagent for each trial performe…

A: We are to discuss the limiting reagent for each trial for given reaction NaOH + MgCl2 → Mg(OH)2 +…

Q: 2) NazCO3(aq) + CaCl2(aq) → 2 NaCl(ag) + CaCO3(8) Calculate the volume (in mL) of 0.200 M Na2CO3…

A: As CaCl2 is present in excess therefore, the amount of product formed depends only on the amount of…

Q: Na,CO3(aq) + CaCl,(aq) → 2 NaCl(aq) + CaCO3(s) Calculate the volume (in mL) of 0.200 M Na»CO3 needed…

A: Given, mass of CaCO3 = 2.00 g molar mass of CaCO3 = 100.09 g/mol => moles of CaCO3 = mass of…

Q: How many moles of Li₂S will be required to completely react with 62.9 mL of 0.100 M Fe(NO₃)₃? 3…

A: Since you gave posted multiple questions with multiple sub-parts, we are entitled to answer the…

Q: When 7.80 mL of 0.500 M AgNO3 is added to 6.25 mL of 0.300 M NH4CI, how many grams of AgCl are…

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.700 M Zn(NO₃)₂ reacts with 23.0 mL of…

A: Number of moles of substance=Concentration of substance x Volume of substanceFor…

Q: Determine the concentration (in M) of excess reactant after 100 mL of 1.26 M AgNO3 react with 100 mL…

A: According to the question, The volume of the AgNO3 = 100 ml = 0.1 L The molarity of the AgNO3 = 1.26…

Q: Calcuate the volume

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.700 M Zn(NO₃)₂ reacts with 31.0 mL of…

A: ZnNO32+2 NaOH→ZnOH2 s+2 NaNO3 aqStength of ZnNO32=20.5x0.700 M1000=0.0143Stength of NaOH=310x0.700…

Q: You are studying the following reaction which occurs in aqueous solution: 2 HNO3 (aq) + Ba(OH)2 (aq)…

A: Step 1:To find the number of moles of HNO3 present before the reaction occurs, we need to use the…

Q: 2) Na,CO3(aq) + CaCl2(aq) → 2 NaCl(aq) + CACO3(s) Calculate the volume (in mL) of 0.200 M CaCl,…

A: Given Mass of caco3 = 2.0 g Molarity of cacl2 = 0.2 M

Q: Answer the following questions for the reaction NiCl₂ (aq) + 2NaOH(aq) → Ni(OH)2 (s) + 2NaCl(aq) How…

Q: Hello Bartelby! Can one of the experts help me answer this two-part question, please?

Q: Using the equation below, how many g of Cu(OH)2 are required to react completely with 26.6 m of a…

Q: How many milliliters of 0.592 M KOH are needed to react completely with 55.0 mL of 0.271 M FeCl2…

A: Mole of a substance is defined mass of substance upon the molar mass of substance moles =mass molar…

Q: None

A: Step 1: In order to determine the moles of generated Fe(OH)2 solid, we must first calculate the…

Q: If 22.5 g of NaOH is added to 0.600 L of 1.00 M Mn(NO3)2, how many grams of Mn(OH)2 will be formed…

Q: How many mL of 1.25 M HCI would react fully with 15.25 mL of 0.836 M Ca(OH)2? 2 HCI + Ca(OH)2 →…

Q: BaCl2 (aq) + NazSO4(aq) → BaSO4 (s) + 2NaCl (aq) How many grams of sodium chloride are produced by…

Q: PC15 (s) + H₂O(l) →→→ POC13 (1) + 2HCl(aq) When 56.22 g of phosphorus pentachloride reacts with…

Q: How many grams of solid Ni(OH)2 are formed when 20.0 thl of 0.550 M aqueous NaOH solution react…

A: Calculation :

Q: Nitric acid reacts with aluminum hydroxide according to the following UNBALANCED reaction:…

Q: Na,CO3(aq) + CaCl2(aq) +2 NaCl(aq) + CaCO3(s) Calculate the volume (in mL) of 0.100 M CaCl, needed…

Q: Find the volume of 0.407 M HCl(aq) required to completely neutralize 1.92 g of Mg(OH)2(s) according…

A: Molar mass of Mg(OH)2 = 58.33 g/mol1.92g of Mg(OH)2 = 1.92/58.33 = 0.033 mole. 1 mole of Mg(OH)2…

Q: Calculate the molarity of a solution of potassium hydroxide if 52 mL is required for the titration…

Q: What volume of 0.125 M HNO3, in milliliters, is required to react completely with 1.30 g of Ba(OH)2?…

A: Note the given balanced equation. 2HNO3(aq) + Ba(OH)2(s) → Ba(NO3)2(aq) + 2 H2O(l) Convert the…

Q: 2 AlCl3 (aq) + 3 Pb(NO3)2 (aq) → 2 Al(NO3)2 (aq) + 3 PbCl2 (s) Calculate how many g…

A: The given balanced chemical equation is 2 AlCl3 (aq) + 3 Pb(NO3)2 (aq) → 2 Al(NO3)2 (aq)…

Q: Calculate the number of milliliters of 0.566 M sodium hydroxide required to precipitate all of the…

Q: Toxic chromate can be precipitated from an aqueous solution by bubbling sulfur dioxide through the…

Q: When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out…

Q: An experimenter reacts 30.0 mL of a BaCl2 solution with excess AgNO3 as shown in the unbalanced…

A: Number of moles =Given massMolar mass

Q: Answer the following questions based on the reaction of 12.6 mL of 0.234 M potassium iodide and 26.8…

A: • The given reaction is 2 KI (aq) + Pb(NO3)2 (aq)→2 KNO3 (aq) +PbI2(aq) • Here we have to calculate…

Q: How many liters of 0.305 M K3PO4 solution are necessary to completely react with mL of 0.0184 M…

A: The question is asking to find the volume of K3 required to react with the given amount of NiCl2…

Q: What is the correct net ionic equation,

Q: What is the minimum amount of 5.1 MH₂SO4 necessary to produce 27.7 g of H₂(g) according to the…

Q: 3.The following reaction takes place as represented by the balanced chemical equation below:…

A: A chemical reaction is a symbolic representation of the conversion of substances to new substances.…

Q: 50.0 mL of 0.999 M ammonium chloride is added to 20.0 mL of 1.21 M mercury (I) nitrate. Mercury (I)…

A: Limiting reagent is the reagent which is consumed in the chemical reaction completely. It decides…

Q: How many grams of Ag₂CO3 will precipitate when excess K₂CO3 solution is added to 44.0 mL of 0.644 M…

A: A balanced chemical equation contain equal number of atoms of each elements on both sides of the…

Q: What is the mass of solute, in grams, in 100. mL of a 1.263 × 10-³ M solution of Na3PO4? Mass of…

A: The mass of a compound can be determined by the number of moles of compound and its molar mass. It…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

t
ot
pt
1 pt
1 pt
1 pt
1 pt
0 1 pt
S
27 at
What volume of 0.125 M oxalic acid, H₂ C₂O4, is required to react with 95.5 mL of 0.717 M NaOH?
H₂ C₂O4 (aq) + 2 NaOH(aq) → Na2 C₂O4 (aq) + 2 H₂O(l)
1 pt
Volume =
1 pt
1 pt
1 pt
Submit Answer
L
Try Another Version
[References]
4 item attempts remaining

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Answer the following questions based on the reaction of 12.6 mL of 0.234 M potassium iodide and 26.8 mL of 0.136 M lead (II) nitrate, based on the balanced reaction below. (MM of Pbl2 is 460.1 g/mol) 2 KI (aq) + Pb(NO3)2 (aq) → 2 KNO3 + Pbl2 (s) (aq) A student performed the experiment and recovered 0.547 g Pbl2. What it the % yield? (Report to 2 dp and no % sign in answer.)
Find the volume of 0.339 M HCl(aq) required to completely neutralize 0.278 g of Al(OH)3(s) according to the unbalanced reaction: HCl(aq) + Al(OH)3(s) → AlCl3(aq) + H2O(l) The molar mass of Al(OH)3 is 78.0 g/mol. Give the answer in mL with 3 or more significant figures.
3. How many milliliters of 0.329 M Barium nitrate are required to precipitate as Barium sulfate all the sulfate ions from 65.0 mL of 1.150 M Aluminum sulfate? Ba(NO3)2(aq) + Al2(SO4)3(aq) → 3BaSO4s) + 2 Al(NO3)a(aq)
Consider the Macmi MgCl₂(aq) + 2NaOH(aq) Mg(OH)₂ (s) + 2 NaCl(aq) A 138.0 mL solution of 0.123 M MgCl, reacts with a 33.32 mL solution of 0.548 M NaOH to produce Mg(OH)₂ ® Identify the limiting reactant. O NaOH NaCl MgCl, O Mg(OH)2 Caclulate the mass of Mg(OH)₂ that can be produced. H mass of Mg(OH)₂: The actual mass of Mg(OH), isolated was 0.445 g. Calculate the percent yield of Mg(OH)2. percent yield: 2 c and NaCl. 80 %
In the reaction below, how many grams of chlorine gas (Cl₂) are needed to react with 5.393 x 1023 molecules of sodium hydroxide? Cl₂(g) + NaOH(aq) → NaCl(aq) + NaClO3(aq) + H₂O(l) What volume (in L) of 0.125 mol/L Ba(OH)2 solution is needed to react completely with 0.200 L of a 0.300 mol/L HNO3 solution according to the following reaction: Ba(OH)2(aq) + HNO3(aq) → Ba(NO3)2(aq) + H₂O(l) ->>
QUESTION 11 A student titrates 26.5 mL of a sulfuric acid solution with 0.750 M NaOH. The color change indicates that it takes exactly 47.9 mL of the NaOH solution for the reaction to go to completion. What was the concentration of the original H₂SO4 solution? (Write your answer in 3 significant figures)? The balanced equation is: H₂SO4 (aq) + 2 NaOH (aq) → 2 H₂O (1) + Na2SO4 QUESTION 12 Metals frequently adopt solid-state structures which can be described is terms of cubic, face-centered cubic or body-centered cubic unit cells with metal atoms located at the lattice points. Ni is face-centered cubic, Fe is body-centered cubic and Ga is simple cubic. Which description below correctly indicates the number of metal atoms per unit cell? OA. Fe 4 OB. Fe 1 OC. Fe 2 OD. Fe 9 OE. Fe 14 NN NN N Ni Ni Ni 4 Ni 14 Ni 9 Ga 1 Ga 4 Ga 1 Ga 8 Ga 8 save all answers.
Toxic chromate can be precipitated from an aqueous solution by bubbling sulfur dioxide through the solution. How many grams of sulfur dioxide are required to treat 1.1 L of 0.12 M chromate? 2 CrO42-(aq) + 3 SO2(g) + 4 H+(aq) → Cr2(SO4)3(s) + 2 H2O(l) Your answer should have 2 sig figs. Molar Masses if needed: H2O 18.02 g/mol, Cr2(SO4)3 392.21 g/mol, SO2 64.07 g/mol
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. How many millimoles of Ba(NO3)2 are there in the solution? How many millimoles of NaIO3 are there in the solution? How many millimoles of NaIO3 are needed to completely react with the Ba(NO3)2? How many millimoles of Ba(NO3)2 are needed to completely react with NaIO3? What is the limiting reagent? What is the excess reagent? What is the concentration of the excess reagent? What is the molar solubility of Ba(IO3)2 in this solution?
Barium sulfate precipitates when aqueous solutions of barium perchlorate and ammonium sulfate are mixed. What is the ratio of the amount of formed precipitate to the amount of the second product (i.e. mol BaSO4/mol NH4ClO4)? Ba(ClO4)2(aq) + (NH4)2SO4(aq) ➜ BaSO4(s) + NH4ClO4(aq) Select one: a.1 b.1/4 c.1/2 d.2
How is HCN the limiting reagent if Ca(OH)2 is producing less?
3) What volume (in milliliters) of 0.1M AgNO3 would be needed to completely react with 2.50 g zinc? Start with the grams of zinc. Zn(s) + 2 AgNO3(aq) = 2 Ag(s) + Zn(NO3)2(aq)