By titration, it is found that 14.7 mL of 0.190 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] M
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![By titration, it is found that 14.7 mL of 0.190 M NAOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
concentration of the HCl solution.
[HCI] =
Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F861073eb-90f0-4339-aab4-71455772cad6%2F9e72da9c-1734-4bf0-96e6-bfcadbada471%2Flf3dpr7_processed.png&w=3840&q=75)
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- A 23mL sample of HCl is titration to phenolphthalein end point with 26.43 mL of a 0.09181 M NaOH standard solution. Calculate the molar concentration of the HCl solution.If a titration net volume for the standardization should be 23.50 mL and a student accidentally one drop past the endpoint (~0.05 mL), will the calculated NaOH concentration (M) be higher or lower than the true value of that solution’s concentration? Explain briefly.Calculate the volume in mL of 0.311 M KOH necessary to titrate 23.38mL of 0.342 M diprotic sulfuric acid, H2SO4 to a phenolphthalein end-point. Report your answer to a precision of 2 decimal places.
- Calculate the volume in milliliters of 0.368 M KOH necessary to titrate 0.0209 moles of acetic acid (HOAc, HC2H3O2) to a phenolphthalein end-point. Report the answer with a precision of two decimal places.For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?The reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq)---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (HNO2) when 40.5 mL of 0.674 M KOH is required to quench 101.0 mL of Nitric acid over phenolphthalein indicator.
- The titration of 20.0 mL of an unknown concentration of H2SO4 (aq) solution requires 50.00 mL of 0.200 M NaOH (aq) solution. Please help me Answer questions (a – d) shown in the photo attached.This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?Give typed solution A student analyzed a CaCO3 antacid tablet by neutralizing the base with an excess of .60 M HCL and back-titrating the excess with .50M NaOH. He recorded the following data: mass of tablet = 1.3g amount of active ingredient CaCO3 per label = 500 mg volume of HCl added: 25 mL initial buret reading : 34 mL final buret reading : 47.4 mL If the concentration of the provided HCl is actually higher than .60M, would the determined mass of CaCO3 in the antacid tablet be too high or too low?
- Calculate the grams of Acetic Acid ( M. W. 60.05g/ mole) in a unknown sample. A sample of Acetic Acid was titrated to the end point using 23.76M NaOH solution. The initial buret reading was 0.6559mL and the final reading was 0.02435mL.A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).A solution of .0490M HCl is used to titrate 29.0ml of an ammonia solution of unknown concentration. The equivalence point is reached when 16.0ml HCl solution have been added. Assume KW is 1.01e-14. What is the pH at the equivalence point
