A 47.90 mL aliquot from a 0.500 L solution that contains 0.480 g of MnSO4 (MW= 151.00 g/mol) required 40.9 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 (MW = 100.09 g/mol) will react with 1.68 mL of the EDTA solution? mass: mg

A 47.90 mL aliquot from a 0.500 L solution that contains 0.480 g of MnSO4 (MW= 151.00 g/mol) required 40.9 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 (MW = 100.09 g/mol) will react with 1.68 mL of the EDTA solution? mass: mg

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: A student weighs out 0.9854 g of Na2CO3 unknown and dissolves it in 25.00 mL of deionized water. A…

A: Answer % of Na2CO3 in the unknown = 54.05% Formulas No.of moles = Given…

Q: Find the pH of the equivalence point(s) and the volume (mL) of 0.447 M HNO3 needed to reach the…

A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…

Q: Consider the titration of 50.00 mL of 0.200 M acetic acid CH,CO,H with 25.00 mL of 0.400 M NaOH. The…

Q: In a reaction 45.0 mL of 0.3M of HC2H3O2 is titrated with 0.2M KOH solution. Ka= 1.8x10^-5 1) what…

A: Answers are explained below.

Q: Calculate the relative amounts (in grams or milliliters) of each buffer component needed to prepare…

A: #1 Given the desired pH of buffer solution = 7.0 Since 7.0 is closest to pKa2 value, we need…

Q: in an experiment, the molecular formula for calcium hydroxide was determined to be Ca(OH)2. In this…

A: Given that : The mass of Ca = 0.050 g The volume of DI water = 150 mL The molarity of HCl = 0.30 M

Q: Which is the best colored indicator to use in the titration of 0.1 M NH3(aq) with 0.1 M HCl (aq)?…

A: Which one of the correct

Q: he Ka of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48 M…

A: Answer - The correct option is (c) The answer for (1) is 30.0 ml. The answer for (2) is 60.0 ml.…

Q: Calculate the number of grams of CaCO3 in 5ml of water that has been titrated with 1.98ml of 0.0100M…

Q: MW (g/mol)-137.99 Buffer 1: 1 M NaH₂PO V 100 mL m(g) Buffer 2: 1 M Na2HPO4 V-100 mL MW (g/mol) 142…

A: The objective of the question is to calculate the-Mass of Monosodium phosphateMass of Disodium…

Q: Titration of (4.77300x10^-1) grams of monoprotic weak acid (dissolved in KCl) required…

A: Given: Mass of weak acid = 4.77300x10-1 gram Concentration of NaOH = 1.965 x 10-1 M Volume of NaOH…

Q: 0 mL of a H₂SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint…

A: Molarity is defined as number of mole of solute divide by volume of solution in liter

Q: Want in Tris-PMSF Buffer, pH = 8.60 10.0 mL 10 mM Tris ( 100 mM, Tris Stock, pH 8. G0) mL 0.5 mM BME…

A: Buffer solution hs two major components i.e. weak acid and its conjugate base. This mixture tends to…

Q: If a 35.0-mL water sample required 10.25 mL of 0.0150 M EDTA solution to reach equivalence point,…

Q: A solution of phosphoric acid (H3PO4) with a known concentration of 0.250 M H3PO4 is titrated with a…

A: At third equivalence point, all the H3PO4 molecule get converted to PO4-3 i.e complete…

Q: A 25.4mL sample of 0.156 M HCl is titrated with 0.249 M NaOH. Calculate the pH after the addition of…

Q: 50mL of 0.025 M HF is titrated with 0.045 M NaOH. a) What amount of NaOH is required for…

A: amount of NaOH is required for equivalency point = 27.77 mL

Q: In the titration of a 30.0-mL sample of 0.115 M H2C6H6O6 with 0.130 M LIOH, where Ka, H2C6H6O6 =…

A: Half equivalence point means the concentration of acid and salt are equal ([Acid] = [salt]).…

Q: Which of the following indicators will be the most appropriate to be used for the titration of 25.0…

A: When we titrate 25.0 mL 1.0 M Na2CO3, with 1.0 M HCI titrant, up to first equivalence point CO32-…

Q: The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is

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

Q: What is the pKa of the 0.225 g sample of a solid acid titrated with 0.100 M KOH? 14 12 10 8. 4. 10…

A: In this question, we want to determine the pKa of acid. You can see the details explanation and…

Q: 41.9ml sample of a 0.593M aqueous nitrous acid solution is titrated with a 0.349M aqueous sodium…

A: Buffer formed by the combination of mixture of weak acid and salt of weak acid and strong base.It is…

Q: Which of the following does NOT happen with a weak acid's pKa = pH of the environment? Answers A-D A…

Question

A 47.90 mL aliquot from a 0.500 L solution that contains 0.480 g of MnSO4 (MW = 151.00 g/mol) required 40.9 mL of an
EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 (MW = 100.09 g/mol) will react with
1.68 mL of the EDTA solution?
mass:
mg

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

Step 1: Writing the objective-

VIEW

Step 2: Determining the moles of EDTA-

VIEW

Step 3: Determining the mass of calcium carbonate-

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 15 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

Calculate the pH of the solution:
A 37.1 mL sample of 0.220 M in HZ is titrated with 0.108 M KOH. (for HZ: Ka = 4.4 x 10−7) How many mL of KOH are required to reach the equivalence point?
A 25.00 mL solution of 0.08960 M NaI is titrated with 0.05040 M AgNO3. Calculate pAg+ following the addition of the given volumes of AgNO3. The ?sp of AgI is 8.3×10−17 .35.20 mLpAg+= ?epAg+= 46.40 mLpAg+=
A 0.2014 g of the primary standard Na2CO3 (105.99 g/mol) required 37.00 mL of HCl (36.45 g/mol) to reachthe yellow endpoint of the bromocresol green indicator. Give the balanced chemical equation for the standardization of the HCl titrant and calculate the standardized concentration of HCl.
12.) 0.120 g of an unknown diprotic acid is titrated with 0.110 M NaOH. The first equivalence point occurred in the titration at a volume of 7.20 mL of NaOH added; the second equivalence point occurred at a volume of 14.40 mL of NaOH added. What is the molecular weight of the diprotic acid? diprotic acid molecular weight = g/mol %D
You're asked to find the concentration of Ca2+ in an unknownsolution of calcium carbonate (CaCO3). You titrate 50.0 mL of the unknown solution with 0.0250M EDTA. It requires 16.85 mL of EDTA to reach the equivalence point. Determine [Ca2+] of theunknown solution, in ppm. Recall that ppm (parts per million) is equal to mg/L. Thank you!
None
em/forms/d/e/1FAlpQLSd7Qir0XcW1yfDw7IHKj570x6qm-viAIM52kDShE8L98ycvaC In titrating 10 ml of 0.1 N HA (pKa-D4),the pH after the addition of 12 ml 0.1N NAOH is 3.69 11.2 13.8 13.21 12.31 4.50 10.3 13.3 11.3 O2.69 Submit
a) Calculate the pH of a buffer solution made by combining 3.509g of NAOAC •3H,0 to 8.8mL of HOAC (acetic (Sodium acetote trilydrae) then adding this Solurion to 55.6 mL of pure worter (Total Vol. of sol'n= 64.4 mL b) Calculate the pH Of the above buffer sol'n after adding l0 mL of 6.0M of HCI ao C) Calculate the pH of the buffer sol'n from (a) after adding 1.0mL of 6.0M of NoaOHiags
The pK, values for the dibasic base B are pKpi = 2.10 and pK2 = 7.62. %3D %3D Calculate the pH at each of the points in the titration of 50.0 mL of a 0.50 M B(aq) solution with 0.50M HCI(aq). What is the pH before addition of any HCI? pH = What is the pH after addition of 25.0 mL HC1? pH = What is the pH after addition of 50.0 mL HCI? pH What is the pH after addition of 75.0 mL HCI? pH = What is the pH after addition of 100,0 mL HCI? pH =
1) A 1.0L solution of 1.0 M NaF is titrated with 1.0 M HCI, What is the pH of the solution after the addition of 0.00, 0.50, 1.0, and 1.5 L of 1.0 M HCI? The pk, of HF is 3.17. 2) A15L solution of 1.0x10 M HCIO, is titrated with 2.0x10 MCa(OH),. What is the pH of the solution after the addition of 0.00, 0.25, and 0.50 L of 2.0x10 M Ca(OH);? The pk, of HCIO, is 1.96.
1 (a.) Which of the following is TRUE for the titration of a weak base with a strong acid? the equivalence point is at a pH below 7 the equivalence point is at pH 7 the equivalence point is at a pH above 7 the equivalence point is at pH 1 (b.) Which of the following is TRUE for the titration of a strong base with a weak acid? the equivalence point is at a pH below 7 the equivalence point is at pH 7 the equivalence point is at a pH above 7 the equivalence point is at pH 1