Identify the equivalence point of the weak base-strong acid titration curve in the above graph. pH Value 14.0 12.0 10.0 8.0 Weak base 6.0 4.0 2.0 0.0 0.0 10.0 Strong base 20.0 Equivalence point for the strong base 30.0 Volume of HCI Added (mL) 40.0 50.0
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Identify the equivalence point of the weak base–strong acid titration curve in the graph.
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- Advantages of potentiometric titrations over 'classical' visual indicator methods: (select the correct statement(s)). Can be used for colored, turbid or fluorescent analyte solution. Can be used if there is no suitable indicator or if the color change is difficult to visualize. Both answers 1 and 2 are correctSources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration)1. No blank correction Ex _______ET2. Bubbles trapped in the tip of burette: EX ______ ET3. Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX _____ ET2,5 ml volume has taken from an “hypothetic” solution which includes (3+) Sb and (3+) Fe and at the titration with 0.1004 N KMnO4, the wasted amount has found as 16,4 mL. The other 2,5 mL that has taken, has reduced with Zn after that, this 2,5 mL solution has titrates with the same KMnO4 solution solution and the wasted amount is 26,5mL. With these datas find the %concentrations of the ions at the solution.
- A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?A 250.0mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091M NAOH , requiring 29.5ml to reach end point. Determine equivalent weightplease stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10
- 1) The equivalence points of the two titrations curves were not in the same pH range explain why. 2) Using the experimental data at 1/2 the equivalence point volume, calculate the Ka of acetic acid. Volume of NaOH at Equivalence point for HCl Trial = 5.083ml Equivalence point pH for HCl Trial = 6.57 pH 1/2 Equivalence point for HCl Trial = 3.285 Volume of NaOH at Equivalence point for HC2H3O2 = 4.025ml Equivalence point pH for HC2H3O2 Trial = 4.13 pH 1/2 Equivalence point for HC2H3O2 Trial = 2.065While preparing the samples for analysis, you forgot that you already added phenolphthalein indicator so you added some more. What will be its effect in the volume of the titrant needed to reach the endpoint? Select one: A. Increase B. Decrease C. No effect D. Cannot be determined Primary standards are used to determine the exact concentration of the titrant. Based on the criteria of primary standards, which of the following cannot be used as a primary standard? Select one: A.Oxalic acid B. Sodium hydroxide C. Sodium carbonate D. Potassium dichromate During titration, you notice that the retention of the faint pink color is longer than earlier. Your lab partner suggested that you add a “half-drop” to prevent over-titration of the analyte solution. Is it ethical to do the “half-drop” technique? Select one: A. NO. It will cause error in calculations if you forgot to record the volume reading before adding the half-drop. B. YES. No error in calculations will be encountered provided…Using the derived endpoints for both phosphoric acid titrations, calculate theconcentration of the phosphoric acid solution and report the mean value. Vol Mid Point 1st Derivative 3.96 0.089821268 5.91 0.229138878 7.105 0.257152358 8.345 0.562805368 9.025 1.958394009 9.175 4.406074475 9.215 10.52631579 9.27 5.043426253 9.355 4.129394633 9.415 7.738714375 9.465 2.260096883 9.505 13.04347826 9.605 1.258033788 9.8 0.85812357 10 0.845641773 10.25 0.636571666 10.65 0.415019763 11.2 0.31048471 11.95 0.277373275 12.925 0.270438943 13.875 0.273865319 14.55 0.391304348 15.025 0.421607378 15.425 0.567030224 15.7 0.934574579 15.9 0.898689411 16.05 1.831703765 16.125 4.911587269 16.175 4.137715831 16.25 3.061160807 16.325 7.932182234 16.375 6.403162055 16.45 3.070522155 16.55 1.981485334 16.675 1.751612232 16.875 0.8562513 17.075 1.352194716 17.375 0.427848277 17.85 0.434990639 18.475 0.249635948 19.275…
- Chemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Standardization of Titrant Question 7 Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX __ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) Question 8 No blank correction Ex ___ ET Question 9 Bubbles trapped in the tip of burette: EX ___ ET Question 10 Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX ___ ETIm doing a lab for chemistry and need help answering numers 1 and 2 below using the data provided. The molar concentration of the sodium for both is .100M. For your coarse titration, record the following results. initial burette volume reading of NaOH titrant at the start (mL) 0.00 final burette volume reading of NaOH titrant before the color change (mL) 29.05 volume of NaOH solution dispensed (mL) 29.05 volume of HCl solution in the flask (mL) 5.00 1) Calculate the molar HCl concentration using your coarse titration results. For your fine titration, record the following results. initial burette volume reading of NaOH titrant at the start (mL) 0.00 burette volume reading of NaOH titrant at the color change (mL) 30.05 volume of NaOH solution dispensed (mL) 30.05 volume of HCl solution in the flask (mL) 5.00 2)Calculate the molar HCl concentration using your fine titration results.