Select Weak Acid as the analyte in the titration interactive. Analyte, 25.0 ml. Weak Acid, 1.0... Determine the pK, of this weak acid. colortess Indicator No Indicator 14 13.83 pK, = Incorrect PH=2.50 25 50 Titrant Added (mL) Titration Curve Concentration Chart Titrant: Strong Base, 1.0 M MOH 50 0.0 ml + Hd
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- 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: Measured mass of the precipitate 1. Filter paper was dried prior to filtration. EX _____ ET TOPIC: Standardization of Titrant 2. 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) 3. No blank correction EX ______ ETSources 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 ___ ETNa2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
- CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42- should be used so that Ag2CrO4(s) just starts to form at the equivalence point? If a concentration of 0.0010 M CrO42- is used instead, at what concentration of Br- will Ag2CrO(s) just start to precipitate? Do you think this is likely to introduce significant error? The Ksp for Ag2CrO4(s) is 1.2x10-12.A sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930MAdvantages 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 correct
- While 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…Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H2O ⇌ H3O+ + In- Using the results from the experiment, identify which of the reactant/product are responsible for the red and green color of the indicator.Notes: solution turns red after adding acid; solution turns blue/green after adding base RED: ________________________ BLUE/GREEN: ________________________ Why is the color violet/blue at pH near 7? Answer in 1 sentence. Hint: What is the relationship of the species responsible for the observed colors? __________________________________________________________________please 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
- 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)?You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mL2,5 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.