A 10.0 mL aliquot of a 0.200 mol/L HCl solution was titrated with 0.100 mol/L NaOH. what is the pH initial!? What is the pH at the equivalence point?! What is the expected volume to reach the equivalence point?! Draw the titration curve
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A 10.0 mL aliquot of a 0.200 mol/L HCl solution was titrated with 0.100 mol/L NaOH. what is the pH initial!? What is the pH at the equivalence point?! What is the expected volume to reach the equivalence point?! Draw the titration curve
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- Two 21.0 mLmL samples, one 0.100 molL−1HClmolL−1HCl and the other 0.100 molL−1HFmolL−1HF, were titrated with 0.200 molL−1KOHmolL−1KOH. a)What is the volume of added base at the equivalence point for HClHCl? b) -What is the volume of added base at the equivalence point for HFHF? c) Predict whether the pHpH at the equivalence point for each titration will be acidic, basic, or neutral. Predict whether the at the equivalence point for each titration will be acidic, basic, or neutral. neutral for HClHCl, and acidic for HFHF neutral for HClHCl, and basic for HFHF neutral for HFHF, and basic for HClHCl neutral for HFHF, and acidic for HClHCl neutral for both d) Predict which titration c urve will have the lowest initial pHpH. Predict which titration curve will have the lowest initial . HFHF curve HClHCl curve e)Choose a rough sketch of each titration curve.A 10.0 mL aliquot of 0.100 mol/L NaOH solution was titrated with 0.200 mol/L HCl. what is the pH initial!? What is the pH at the equivalence point?! What is the expected volume to reach the equivalence point?! Sketch the titration curveCalculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) (a no KOH added???? (b)20. mL of KOH solution added???? (c)39 mL of KOH solution added???? (d)40. mL of KOH solution added???? (e)41 mL of KOH solution added????
- The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution with 0.0700 M KOH. How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT)A 20.0mL sample of 0.030M formic acid is titrated with 0.015M KOH solution. What is the pH at thefollowing points along the way? a. Before the titration begins b. After addition of 23.0mL KOH solution c. At the equivalence point d. After addition of 45.0mL KOH solutionBuild a titration curve for the following scenarios. Make sure to label your accesses and anyother appropriate pieces of data. Each curve should have a minimum of 4 data points, but youcan use the following to help structure your curvea) Initial pHb) pH at Veqc) pH=pka (if applicable)d) pH when excess titrant is addede) Additional pH point near Veq for Strong Acid/Strong Base titrations (in order to see thesteepness of the slope) OR additional pH point in buffer zone for titrations with a Weakcompound.
- Consider the following titration curve for the titration of maleic acid (HOOC-CH₂=CH₂-COOH) with 0.10 M NaOH. How many equivalent point(s) is (are) present in the titration curve? What is (are) the pH value(s) at the equivalence point(s)? Choose all that applies: 3 4 7 9 Please also estimate the pKa (or pKas) for this curve.25.0 ml of 0.100M NaOH is titrated with HC2H3O2 and 50.0mL of the acid is used to reach the endpoint. e)Would the compound formed at the equivalence point be acidic, basic or neutral? Write a hydrolysis equation for the salt formed in a) to support your answer. f) Which indicator should be used for this titration? g)Sketch a titration curve for this reaction. Label the x and y axes.pH Measurement and Buffer Q1.Substances pH value at 25°C [H+] (mol dm-3) vinegar 2.8 ? fruit juice 3.4 ? antacids 9.2 ? Q2. Show the calculation the volumes of the two solutions (acetic acid and sodium acetate) should be mixed for the preparation of the acetic buffer with pH 4.2 by the Henderson-Hasselbalch equation. Q3 .Solution : Acetic Buffer NaCl Original pH : 4.2 7.2 pH after adding 5 drops of HCl : 4.2 2.7 pH after adding 5 drops of NaOH : 4.2 11.1 Which sample showed little or no change in pH upon the addition of acid and base? Please write an equation and explain briefly.
- A student needs to determine by titration with NaOH the precise %KHP in an unknown sample that is thought to contain approximately 50%KHP. Approximately what mass of sample should the student use in order to use about 20mL of 0.1005 M NaOH to reach the endpoint of the titration?Construct a rough plot of pH versus volume of added base for the titration of 50 mL of 0.045 M HCN with 0.075 M NaOH. Ka = 4.0*10-10 for HCN (a) What is the pH before any NaOH is added? (b) What volume of base, in milliliters, is required to reach the equivalence point? (c) What is the pH at the equivalence point? HopHelpCh17N8(d) What indicator would be most suitable to determine the endpoint?HopHelpCh17N9Weak acid and strong base titration A 20-mL sample of 0.1N HAc was diluted with sufficient water to measure 100mL and titrated with 0.1N NaOH 15 ml, 20 ml and 29 ml - what is the pH of before the titrant is added? - pH after the titrant is added before the equivalence point - pH beyond the equivalence point