A solution is prepared by dissolving 0.6194 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution? _____________ mol/L

A solution is prepared by dissolving 0.6194 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution? _____________ mol/L

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

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 47E

See similar textbooks

Related questions

Q: A 0.3000 g sample of impure Na2CO3 requires 36.31 mL of a 0.1075 M HClO4 solution to reach the end…

A: Molarity of HClO4 = 0.1075 M Volume of HClO4 = 36.31 mL = 0.03631 L Mass of sample = 0.3000 g We…

Q: How many grams of Ag2CrO4 will precipitate if excess K2CrO4 (aq) is added to a 41.5 mL of 0.816M…

A: Ag2NO3 is limiting reactant. and K2CrO4 is given in excess...

Q: Molarity calculations- A student adds 1.55g AlCl3 to 125.00 mL water. Then, the student adds 40.00mL…

A: In this question, We have to Calculate the [Cl-] in the final solution when a student adds 1.55g…

Q: True or False? When 100.0 mL of 2.4 M hydrochloric acid is added to 500.0 mL of water, the…

A: molarity is defined as no of moles of solute devided by volume of solution in liter.

Q: 12. AU.S. penny has a mass of 2.500 g and is composed of 2.5% copper and 97.5% zinc (by mass). How…

Q: Refer to picture below. What is the pAg of the solution after addition of 5.00 mL AgNO3?

A: According to our policy, only the first question is solved and if the answers to others are required…

Q: Mg(OH)2(s) + 2HCl(aq) --> MgCl2(aq) + 2 H2O(l) Use the equation above to answer the following.…

Q: Nickel (II) Nitrate solution is a pretty green color. If you were to add 12.0 grams of solid nickel…

Q: Consider the balanced equation of KI reacting with Pb(NO3)2 to form a precipitate. 2 KI (aq) +…

Q: How many grams of Ag2CO3 will precipitate when excess (NH4)2CO3 solution is added to 44.0 mL of…

A: Given, the chemical reaction as follows, 2AgNO3(aq) + (NH4)2CO3(aq) => Ag2CO3(s) + 2NH4NO3(aq)…

Q: A technician tritated a vinegar sample. Data Below: Concentration of NaOH = 0.500 M Final buret…

A: Given : Concentration of NaOH = 0.500 M Final buret reading = 32.46 mL Initial buret reading =…

Q: (1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she…

A: (1)The relationship between mass, moles and molar mass of a substance is given by,

Q: What is the concentration of an original Li2CO3 solution, if 30.0 mL of the solution is diluted to a…

A: We can determine the original concentration from the dilution law: V1 × S1 = V2 ×S2 Where V1 =…

Q: The moles of a substance in solution depends on how much solution there is (the volume) and how much…

A: We use the below formula from part#(a) to find the moles of sodium carbonate in the desired diluted…

Q: Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid (below). A…

Q: Part 9: Balance the equation Substitute into the formula with units. Show your answer with units Use…

Q: uppose you need 0.14L of a 0.06M solution of NiCl₂, but all you have is a solution that is a…

Q: Redox Titration 2 KMnO4 + 5 (COOH)2 + 3 H2SO4 -------> 10 CO2 + 2 MnSO4 + K2SO4 + 8 H2O

A: It is the redox titration between oxalic acid and potassium permanganate solution. Here at first we…

Q: B. Use the equation to calculate the following: K,CO3(aq) + 2 HC,H¿O,(aq) → 2 KC,H¿O¿(aq) + H,O(!) +…

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

A: Given information: Volume and concentration of CrO42- are 9.8 L of 0.12 M The reaction is…

Q: What volume (in mL) of 0.200M Na3PO4 solution is necessary to completely react with 99 mL of 0.10 M…

A: molarity of CuCl2=0.10MVolume of CuCl2=99ml=0.099LNo. of moles of CuCl2=molarity×volume in…

Q: A 46.2-mL, 0.568 M calcium nitrate [Ca(NO3)2] solution is mixed with 80.5 mL of 1.396 M calcium…

Q: What is the final concentration of a solution made by mixing 160.0 mL of 1.50 M KNO3 with enough…

Q: 6. A student does not remove the air bubble from the tip of the burette before standardizing the…

Q: Calculate the molarity of a solution that contains 324 grams of KNO3 (molar mass of KNO3 =86 g/mole)…

A: Molarity ( M ) : it is defined as the number of moles of solute present in dissolved state in one…

Q: Suppose 30.0 ml. of 0.100 M Pb(NO-h is added to 60.0 ml. of 0.150 M KI. How many grams of Pbl2 will…

A: Solutions- Given data- 0.100M Pb(NO3)2, 0.150M KI, Volume = 30.0 ml Pb(NO3)2, 60.0 ml of KI.

Q: Suppose that 3.50 g of potassium chromate is added to 75.0 ml of 0.250 M magnesium nitrate. 1. What…

A: Here we are required to find the molar concentration of potassium chromate and mass of potassium…

Q: 3NaOH= H3PO4----> Na3PO4+ 3H20 A 41.0ml sample of NaOH solution of unknown concentration requires…

A: Given, 24.3 mL of 0.150M H3PO4 no. Of moles of H3PO4= 0.0243 L × 0.150M No. of moles of H3PO4 =…

Q: A 1.000-L sample of polluted water was analyzed for lead (II) ion, Pb2+, by adding an excess of…

A: -> weight of lead (2) sulphate = 208.4 mg = 0.208 g (1 g = 1000 mg)

Q: Part A A solution of NazCO3 is added dropwise to a solution that contains 1.04 x 10 ?mol L' Fe²+ and…

A: Given: Concentration of Fe2+ ions = 1.04 X 10-2 M And concentration of Cd2+ ions = 1.57 X 10-2 M

Q: 36. Zinc reacts with HCl to produce ZnCl₂ and hydrogen gas H₂: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g).…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 5. 14.0 g of cobalt(III) chloride are mixed with water to give 250.0 mL of solution. 15.00 mL of…

Q: 41.9 ml. of 0.151 M NAOH was needed to neutralize 50.0 mL of an H2S04 solution. What is the…

A: Sulfuric acid reacts with sodium hydroxide to form sodium sulfate and water. The equation for the…

Q: Volume of HCL sample = 15ml Molarity standardized NaOh solution = .09929 Initial buret reading =…

A: Given information, Molarity of standardized NaOH solution (M1) = 0.09929 M Volume of NaOH used (V1)…

Q: A 2.00 g sample of KCl is dissolved in 38.0 mL of water. The resulting solution is then added to…

A: Given that - Mass of KCl = 2.00 g Volume of water = 38.0 mL CaCl2 Molarity = 0.320 M Volume of…

Q: 13) How many milliliters of 0.250M AgNO3 would be needed to react exactly with 20.0g of NaCl? pure…

A: Silver nitrate reacts with sodium chloride to form silver chloride and sodium nitrate. The equation…

Q: Molarity of unknown oxalate solution, M: Average concentration of oxalate…

A: The The question is based on the concept of titrations. we are titrating a oxalic acid with a…

Q: Sodium lactate, NaC3H5O3, has uses in medicine to treat low blood pH and in soaps to create moisture…

A: Given, mass of sodium lactate = 9.01 g Volume of the solution = 0.250 L Concentration of sodium…

Q: A 35.0 mL volume of ammonia (NH3) household cleaner needs 53.75 mL of 0.300 M HNO3 to completely…

Q: ou may want to reference Pages 306 - 308) Section 9.5 while completing this roblem. Part A etermine…

A: As we are to prepare a solution using stock solution , hence We will use dilution equation :…

Q: Suppose 6.93 g of solid Mg(OH)2 is added to 27.1 mL of 0.510 M H2SO4 solution. What will the…

Q: Calculate the molarity of a sulfuric acid solutions (H2SO4)

Q: What is the maximum mass of barium sulfate that can be produced from a 350.0 mL of a 0.125 M barium…

Q: P: Dilution Calculations H115 mL of a 12.0 M HCI solution is diluted to 2.00 L, what is the molarity…

A: Solution : Dilution is the process of decreasing the concentration of solute by adding more…

Q: Calculate the milligrams of Cl (35.453 g/mol) in a 3.03 g sample of cleaning solution containing…

A: Given information:Weight percentage of NaOCl = 22.1 %Molar mass of NaOCl = 74.44 g/molMolar mass of…

Q: If 750.0 mL of a 0.750 M-H3PO, solution is be diluted to a volume of 1.00 L, what is the…

A: For the original H3PO4 solution : Molarity, M1 = 0.750 M Volume, V1 = 750 mL For the new diluted…

Q: In the following balanced reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) 10.9 g of KI…

A: Given: Molarity of Pb(NO3)2 = 0.193 mol L-1 Volume of solution = 0.200 L

Q: A NC Residency Deter. +Scholarships - Goo. wh ccsf Read [References] Use the References to access…

A: For dilution , M×V = constant

Q: Suppose 30.0 mL of 0.100 M Pb(NO3) is added to 60.0 mL of 0.150 M KI. How many grams of Pbl2 will be…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Question

A solution is prepared by dissolving 0.6194 g oxalic acid (H₂C₂O₄) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution?

_____________ mol/L

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Molarity

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

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

Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
You made 100.0 mL of a lead(II) nitrate solution for lab but forgot to cap it. The next lab session you noticed that there was only 80.0 mL left (the rest had evaporated). In addition, you forgot the initial concentration of the solution. You decide to take 2.00 mL of the solution and add an excess of a concentrated sodium chloride solution. You obtain a solid with a mass of 3.407 g. What was the concentration of the original lead(II) nitrate solution?
Quantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…
A sample of pure sodium oxalate weighing 0.1050 g is ignited [Na2C2O4 (s) --> Na2CO3 (s) + CO (g)] and the resulting product requires 15.00 mL of a solution of H2SO4 for complete neutralization. What is the normality of the acid? MM of Na2CO3 = 106.0 g/molMM of Na2C2O4 = 134.0 g/molMM of CO = 28.01 g/molMM of H2SO4 = 98.08 g/mol
Vitamin C, ascorbic acid, is an essential nutrient that helps the immune system fight off diseases. One way to consume vitamin C is to eat citrus, like oranges. Ascorbic acid reacts with sodium hydroxide according to the following reaction: HC6H7O6(aq)+NaOH(aq) = NaC6H7O6(aq)+H2O(l) The average orange produces 125.0 mL of juice. A 125.0 mL sample of orange juice required 34.0 mL of 0.0100 M NaOH to complete the reaction. a. What is the concentration of ascorbic acid in the orange juice? b. An adult should consume approximately 90.0 mg of vitamin C a day. How many milliliters of orange juice should someone drink to reach the recommended amount of vitamin C?
What mass of Fe(OH)3 (MW = 106.87 g/mol) will be obtained when 100. mL of 0.240 M FeCl3 (MW = 162.2 g/mol) is mixed with 98.2 mL of 0.263 M NaOH (MW = 40 g/mol)? (Answer format x.xx - 2 decimal places - no units) Consider this balance equation: FeCl3(aq) + 3NaOH(aq) ---> Fe(OH)3(s) + 3NaCl(aq)
naco3(aq) + cacl(aq) ----- 2nacl(aq) + caco3(s) calculate the volume (in mL) of 0.100M cacl needed to produce 1.00g of caco3(s) there is an excess of naco3 molar mass of calcium carbonate = 100.09 g/mol volume of calcium chloride = ? mL
Analysis shows that a 2.750 mL sample of a diprotic acid reacts completely with330.0 mL of 0.2000 M KOH solution. What is the molar mass of the unknown acid? (density of unknown diprotic acid = 1.200 g/mL)
The Original volume of unknown NaCl solution = 98.407mL The concentration of Ag + within the 10 mL unknown NaCl solution after AgCl is added [Ag+] = 4.71370e^-10 Calculate Calculate the mass of NaCl in the 10 mL unknown solution. Show your work.? Hint: mole = molarity x L; mass = mole x molar mass AgCl(s)⇌Ag+(aq)+Cl−(aq) Ksp=[Ag+][Cl−]
Refer to picture below. What is the pAg of the solution after addition of 5.00 mL AgNO3? What is the pAg of the solution after addition of 10.00 mL of AgNO3? What is the pAg of the solution after addition of 15.00 mL of AgNO3?
A technician tritated a vinegar sample. Data Below: Concentration of NaOH = 0.500 M Final buret reading = 32.46 mL Initial buret reading = 23.81 mL Volume of Vinegar tested: 10.00mL a) What was the molarity of acetic acid in the vinegar sample? b) What was the mass percent of acetic acid in the vinegar sample?
A 100.0 mL 0.500 M NaOH solution is made available for a general chemistry class. From this, Woonie transferred a 25.0 mL portion to his own 50.0 mL volumetric flask and diluted it to mark with water. Which of the following statements is false? Select one: A.The 100.0 mL solution has more moles of NaOH than the 25.0 mL portion. B.The 25.0 mL portion has equal moles of NaOH with the 50.0 mL solution. C.The 100.0 mL solution has equal concentration of NaOH with the 25.0 mL portion. D.The 25.0 mL portion has lower concentration of NaOH than the 50.0 mL solution.