Q: AIC13 NaBH4 PBr3
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- A student àdds a small amount of phenolphthalein to an erlenmeyer flask, and it changes to pink when he adds the base, sodium hydroxide. What is phenolphthalein considered to be? a titrant an indicator a quotient an isotitrate an analyteA mixture containing KCl and NaBr was analyzed by Mohr's method. A mass of 0.31011 g of the mixture was dissolved in 50 mL of water, the Na2CrO4 indicator was added, and it was titrated with a 0.11011 mol/L AgNO3 solution. The endpoint was 36.011 mL. What are the % m/m concentrations of KCl and NaBr in the mixture?+ NaOCI NaOH H₂O ?
- (a) The sodium ion did not take part in this chemical reaction. What do we call such an ion? (b) Draw a simple diagram which shows how the sodium ion mixes with water in solution. What do we call this physical process?(b) Sodium hydroxide reacts with propanoic acid in the following equation: NaOH + CH3CH,COOHCH3CH2COONA + HLO A buffer solution is formed when sodium hydroxide is added to an excess of aqueous propanoic acid. (i) Calculate the number of moles of propanoic acid in 50.0 cm of 0.125 mol dm aqueous propanoic acid. (ii) Use your answers to part (b)(i) to calculate the number of moles of propanoic acid in the buffer solution when 2.00 cm' of 0.500 mol dm aqueous sodium -3 hydroxide are added to 50.0 cm' of 0.125 mol dm aqueous propanoic acid. ) Hence calculate the pH of this buffer solution at 298.15 K.Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 15.15 mL of 0.250 M NaOH to reach the phenolphthalein end point. What is the NORMALITY of acetic acid? choices 0.250 1.24 0.808 0.758 0.00310
- Can you please help me with a, b, c and d A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution. d) What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH has been added to only 100.0 cm3 of this buffer?Mr. Clean recently bought a laboratory-grade sodium carbonate from a chemical company known as Brand X. He was supposed to use it in the production of detergents. Unfortunately, he was scammed by the company. He suspected that he purchased a crude sodium carbonate so he tasked the Quality Assurance Department to determine the components of the purchased chemical. The chemist assigned to analyze the sample used double indicator method. For the standardization of HCl titrant, 0.1025 g Na2CO3 of 99.5% purity (FW: 106.00) required 8.20 mL of the titrant to reach the phenolphthalein endpoint. FW: NaOH (40.00), NaHCO3 (84.01), Na2CO3 (106.00) a. What is the molarity of the titrant? The chemist obtained a 3.150 g sample and dissolved it in distilled water to produce a 50.0 mL solution. An aliquot of 10.00 mL was obtained and diluted in a 100.0 mL volumetric flask. A 50.00-mL aliquot of the diluted sample was taken and it required 25.70 mL of titrant for the methyl orange endpoint, while…it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL Volume NaOH used ________mL ________mL ______mL Moles NaOH _______M ________M _________M…
- it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL what Volume of NaOH is used ?A chemistry student weighs out 0.379g of citric acid H3C6H5O7, a triprotic acid, into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M 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.Potassium permanganate (KMnO4) standard solution is prepared by dissolving 1.58 grams of potassium permanganate salt in 1.0 L of distilled water. Adjustment of this solution is done with sodium oxalate (Na2C2O4). 12 mL of this solution was spent in the titration of 0.0501 g sodium oxalate in acidic medium. Calculate the true molarity (M) of the potassium permanganate solution. 2MnO4 + 5C204²- +16H+. 2 Mn²+ +10 CO2 + 8 H2O
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