A solution of tartaric acid (H2C,H,O6) with a known concentration of 0.155M H;C,H406 is titrated with a 0.425 M NaOH solution. How many mL of NaOHare required to reach the second equivalence point with a starting volume of 70.0mL H,C4H,O6 , according to the following balanced chemical equation:H2C4H,O6 +NaOH -Na,C4H,O6 + 2 H20 STARTING AMOUNTADD FACTORANSWERRESET*( )10000.4250.0010.0217212.825.50.15510.051151.1|5.11 х 10470.0M H2C,H,O6g NaOHLH,C,H,O6mol NaOHmol H2C4H,O6mL NaOHM NaOHmL H2C,H4O6L NAOHg H2C,H,O6

Given, H2C4H6O6+2NaOH→Na2C4H4O6+2H2OK. Concentration of tartaric acid = 0.155M Concentration of…

A solution of tartaric acid (H2C,H,O6) with a known concentration of 0.155 M H2C,H,O6 is titrated with a 0.425 M NAOH solution. How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H;C,H,O6 , according to the following balanced chemical equation: H2C,H,O6 + 2 NaOH – NazC4H4O6 + 2 H2o

A solution of tartaric acid (H2C,H,O6) with a known concentration of 0.155 M H2C,H,O6 is titrated with a 0.425 M NAOH solution. How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H;C,H,O6 , according to the following balanced chemical equation: H2C,H,O6 + 2 NaOH – NazC4H4O6 + 2 H2o

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

Similar questions

A student performed titration to determine the concentration of citric acid with potassium permanganate solution. The net ionic equation is as follows: 5C6H8O7 + 18MnO4- + 54H+ → 30CO2 + 47H2O + 18Mn2+ The concentration of potassium permanganate soluiton is 0.266 M. The volume of lemon juice is 25.00 mL. The titration consumed 17.6 mL of potassium permanganate solution to reach the endpoint. Determine the moles of citric acid in the lemon juice sample.
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of potassium hydrogen phthalate (C8H5O4K, M = 204.22 g/mol). In the titration 34.67 mL of NaOH solution is required to react with 0.1082 g C8H5O4K to reach the equivalence point. a) Calculate the concentration of the sodium hydroxide solution. Potassium hydrogen Phthalate = 0-10829, Molar mass of KMP=204-22 Hales of KMP = Mass 0.10829 g/mol Mm 6.000529 mal 204229/Mal Concentration of NaOH = Males = = of volume of Naot (L) = 0-000529 mal 34-67 mе onl ها NaOH (mal) = 0.000015258 mal/L 0.015M b) This solution of sodium hydroxide is used for another titration. A sample of 10.0 mL of HCI is neutralized using 22.1 mL of sodium hydroxide solution. Calculate the concentration of the HCI solution. sodium hydroxide 222.1 ml, Nal100
This is another titration question. When 35.00 ml of phosphoric acid of unknown concentration is titrated with 1.025 M NaOH, and 18.75 ml of NaOH is required to reach the endpoint, what is the molarity of the phosphoric acid? The reaction is: H3PO4 (aq) + 3 NaOH (aq) → Na3PO4 (aq) + 3 H2O (l)
A chemistry graduate student is given 250. mL of a 1.50M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 1º. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.84? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?
Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
Consider the following balanced chemical reaction: H2SO4 (aq) + 2 KOH (aq) ------------> K2SO4 (aq) + 2 H2O (l) What volume, in L, of 0.200 M KOH solution is required to completely react with 2.50 L of 0.400 M H2SO4solution?
A https://app.101edu.co Question 14 of 15 Submit A solution of phosphoric acid (H,PO,) with a known concentration of 0.250 M H,PO, is titrated with a 0.800 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H,PO, according to the following balanced chemical equation: Н,РО, + NaOH > Na PO, + з но 3 4 STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.800 6.75 x 104 2 1 0.250 0.0675 22.5 1000 3 67.5 7.50 72.0 0.001 43.2 LH,PO, mol NaOH M H,PO, g NaOH L NAOH mL H,PO, mL NaOH M NaOH g H,PO, mol H,PO, +
Use the following balanced chemical equation to answer the below question: 2H&PO4 (aq) +3Mg(OH)2 (aq) 6H2O m + Mg3(PO4)2 (s) The titration of a 14.0 mL sample of H3PO, requires 3.51 mL of 0.400 M Mg(OH)2 to reach the equivalence point. What is the concentration of H3PO,?
A student measures that it takes 7.21mL of 0.326 M NaOH (aq) solution to reach the first equivalence point of a titration of 100.0 mL of phosphoric acid solution. He also notes that it takes a total of 14.40 mL of 0.326 M NaOH (aq) solution to reach the second equivalence point. What is the concentration of the phosphoric acid solution?
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True