A sample of hydrochloric acid is standardized using sodium bicarbonate. The balanced chemical reaction is given below: HClag) + NAHC03(ag) + CO212) + H20) NaCl (aq) Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. O 0.00015 M 0.15 mol O 0.00015 mol O 0.15 M

A sample of hydrochloric acid is standardized using sodium bicarbonate. The balanced chemical reaction is given below: HClag) + NAHC03(ag) + CO212) + H20) NaCl (aq) Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point. O 0.00015 M 0.15 mol O 0.00015 mol O 0.15 M

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 chemistry student weighs out 0.0827 g of phosphoric acid (H,PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0600M NaOH solution. Calculate the volume of NAOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL FEB 19 ... MacBook Air DII 80 888 F10 F7 FB F9 F4 F3 %23 %24
A student titrates a 35.00 mL sample of 0.0100 M sodium hypochlorite (NaClO), a salt containing the conjugate base of hypochlorous acid (HClO, Ka = 3.0 x 10-8), with 0.0125 M HCl. NaClO(aq)+ HCl(aq) → NaCl(aq)+ HClO(aq) Determine the pH after 12.00 mL of HCl has been added.
Calculate the concentration of the hydrochloric acid if a 20.00 mL sample is titrated withstandard sodium carbonate solution.2 HCl (aq) + Na2CO3 (aq) → H2O (l) + CO2 (g) + 2 NaCl (aq)The titration required 10.00 mL of 0.250 mol/L sodium carbonate to neutralize the acid.
A student is given 0.716 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.430 M NaOH. The equivalence point is reached when 37.0 mL are added. Answer the following questions to determine the identity of the unknown acid. -How many moles of NaOH are consumed? Moles of NaOH = ____ mol -How many moles of H+ acid are available to react if the acid is H2C2O4? 0.0403 mol NaOH Moles of H+ from H2C2O4 = ___ mol -How many moles of H+ are available to react if the acid is H3C6H5O7? 0.0403 mol NaOH 0.0573 mol H+ from H2C2O4 Moles of H+ from H3C6H5O7 = ___ mol
To increase the acidity of soil, you can add peat, which contains a complex acid mixture known as humic acid, a diprotic acid (two acidic protons). The complexity of the humic acid makes it difficult to determine how acidic you are making the soil. You decide to use a titration to get a better measure. If a titration of an unknown sample of humic acid required 3.68 mmols of NaOH, how many mmols of humic acid were present in the unknown sample?
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
In the following acid-base titration experiment HNO3 (aq) + KOH (aq) ---------> KNO3 (aq) + H2O(l) What is the molarity of the KOH solution if 18.2 mL of 0.16 M HNO3 was used to neutralize 24.0 mL of KOH?
The iron content of iron ore can be determined by titration with K₂Cr₂O₇ according to the equation 14H⁺(aq) + Cr₂O₇²⁻(aq) + 6Fe²⁺(aq) → 6Fe³⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l) Diphenyl amine is used as an indicator as it changes color from green to purple when the endpoint is reached. A sample of iron ore with a mass of 3.255 g was dissolved with HCl and then treated with a reducing agent to convert any Fe³⁺ in the ore to Fe²⁺. Titration with 0.0645 M K₂Cr₂O₇ solution required 45.65 mL of the solution to reach the endpoint. The molar mass of Fe is 55.85 g/mol. Calculate the mass percent iron in the ore.
An analytical chemist weighs out 0.108 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1300M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 25.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. 0 g mol x10
A chemistry student weighs out 0.106 g of ascorbic acid (H,C,H,O), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NAOH solution. Calculate the volume of NAOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL 19 MacBook Air DII 888 F6 F7 F8 F4 F5 F3 &
Calculate the molar concentration HCl when 250 mL of 0.10 M HCl is mixed with 150 mL of 0.10 M NaOH in a beaker. HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
A 10.00-mL sample of sulfuric acid, H2SO4, is titrated with 0.2760 M NaOH solution. If the titration requires 32.50 mL of the NaOH solution, what is the molar concentration of the H2SO4 solution? The acid-base reaction occurs as follows: H2SO4(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(l)