An analysis was done on 3 unknown samples (NAOH, Na2CO3 and NaHCO3) using double indicator method. A 5.0 mL sample was used foreach analysis and a single burette employing CONTINUOUS TITRATION with 0.0 ml. as INITIAL READING. Phenolphthalein and methylorange indicators were used respectively and a standard solution of HCl with a concentration of 0.4875 N was used. Data from the analysis isshown on the table below:SAMPLEFINAL BURETTE READING in mLMoPp5.812.65.815.8B15.824.7NOTE: Sample A was analyzed first followed by Samples B and C. NO REFILL OF ACID WAS DONE.MW: NAOH 40, NazCO3 106, NAHCO3 84WHAT IS THE IDENTITY OF SAMPLE A?O NagcosONazc0s and NaHCOsO NaOHONazCOg and NaOH

Neutralization reactions of all three possible compounds are: NaOH + HCl ------> NaCl + H2O…

An analysis was done on 3 unknown samples (NaOH, Na2CO3 and NäHCU3) USIng each analysis and a single burette employing CONTINUOUS TITRATION with 0.0 ml. as INITIAL READING. Phenolphthalein and methyl orange indicators were used respectively and a standard solution of HCI with a concentration of 0.4875 N was used. Data from the analysis shown on the table below: FINAL BURETTE READING in mL Pp SAMPLE Мо A 5.8 5.8 12.6 15.8 15.8 24.7 NOTE: Sample A was analyzed first followed by Samples B and C. NO REFILL OF ACID WAS DONE. MW: NAOH 40, NazCO3 106, NaHCO3 84 WHAT IS THE IDENTITY OF SAMPLE A? O Nazcos ONazcoy and NaHCOy O NaOH NazCOs and NaOH

An analysis was done on 3 unknown samples (NaOH, Na2CO3 and NäHCU3) USIng each analysis and a single burette employing CONTINUOUS TITRATION with 0.0 ml. as INITIAL READING. Phenolphthalein and methyl orange indicators were used respectively and a standard solution of HCI with a concentration of 0.4875 N was used. Data from the analysis shown on the table below: FINAL BURETTE READING in mL Pp SAMPLE Мо A 5.8 5.8 12.6 15.8 15.8 24.7 NOTE: Sample A was analyzed first followed by Samples B and C. NO REFILL OF ACID WAS DONE. MW: NAOH 40, NazCO3 106, NaHCO3 84 WHAT IS THE IDENTITY OF SAMPLE A? O Nazcos ONazcoy and NaHCOy O NaOH NazCOs and NaOH

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 37QAP: Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at...

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Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
A sample containing the amino acid alanine, CH3CH(NH2)COOH, plus inert matter is analyzed by Kjeldahl method. A 2.00 g sample is digested, the ammonia is distilled and collected in 50.0 ml of 0.150 M H2SO4, and a volume of 9.0 ml of 0.100 M NaOH is required for back titration. Calculate the percent alanine in the sample.
Na2CO3 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
UEid- base tit ration the Consentrat ion of ammonia Solution excess HCL was titrated ith o.07om Na, cO3 Solutian. The volume of Na, Coz Solution reguired was 15.50 ml using the following eguations: 2HCLem> + Na, COgcaps CO2 Cays + HzO1) t NaCL Calculate the concentration (molarity and ppm) of ammonia in the Original Solution.(MM of NHzis 17.031.9/4) 10.0 was by of o.10OMI HCE to Then
A solution of HCl was titrated against sodium carbonate. What is the titer for Trial 1 in the given data? T2 0.3562 0.3479 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (ml) Vol HCI used (ml) 35.10 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L) A
1) What is the reason 2) In order to determine the hardness of water, 100 mL sample is taken. After neutralizing the sample, pH 10 buffer solutions and Erichrom black-T indicator are added. This sample is titrated with 10.7 mL of the solution containing 3.7225 g EDTA in 1 L distilled water. Calculate the hardness of water in terms of considering the amount of CaCO3 present in the sample. (Mwt Ca:40 g/mole, O:16 g/mole, C:12 g/mole, EDTA: 372,25 g/mole)
I made some titrations and the calculated molarity of HCI was 0.096, 0.097 and 0.098. The nomical concentrsrion of HCl is 0.1. How can I explain my results by comparing it to the nominal concentration if my confidence intervals don't include the nominal concentration?
A 0.5843-g sample of a plant food preparation was analyzed for its N content by the Kjeldahl method, the liberated NH3 being collected in 50.00 mL of 0.1062 M HCl. The excess acid required an 11.89 mL back-titration with 0.0925 M NaOH. Express the results of this analysis in terms of (a) %N (b) %urea, H2NCONH2 (c) %(NH4)2SO4 (d) %(NH4)3PO4
50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the presence of phenolphthalein indicator, the acid consumption is 15 mL. Then, the titration is continued by adding bromocresol green indicator, and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; NazCO3: 106 g / mol)
The amount of CaCO3 in an antacid tablet was determined by back titration. An excess of HCl (50mls of 1.0M HCl) was added to four powdered tablets (total massof tablets 2.110g) and left overnight. The next day, 10ml aliquots of the solution wastitrated against 0.2M NaOH. An average titre value of 16.55mls was determined.Determine the amount of CaCO3 present in one tablet; express your answer as g/tablet and as %wt/wt.