A 0.33 g sample of an unknown tribasic sodium salt (symbolized as Na3X) is titrated to...
A 0.33 g sample of an unknown tribasic sodium salt (symbolized as Na3X) is titrated to the endpoint using 32.33 mL of 0.108 M HCl. Na3X(aq) + 3 HCl(aq) → H3X(aq) + 3 NaCl(aq)
Calculate the molar mass (g/mol) of the unknown.
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A 0.33 g sample of an unknown tribasic sodium salt (symbolized
as Na3X) is titrated to...
25mL of an unknown sodium carbonate and sodium hydroxide mixture reacted with 10mL of .5M SrCl2 is titrated with 1M HCl...
25mL of an unknown sodium carbonate and sodium hydroxide mixture
reacted with 10mL of .5M SrCl2 is titrated with 1M HCl
Using the following endpoints determine (a) the number of moles
of NaOH and (b) the number of moles of Na2CO3. (Show work)
Endpoint 1: 13.2mL HCl used
Endpoint 2: 12.9mL HCl used
To the first endpoint: (1) HCI(aq) + NaOH (aq) NaCl(aq) + H20(0) Between the first and second endpoints: (2) 2 HCl(aq) + SrC03(s)SrCl2(aq) + H20() + CO2(aq)...
A 0.4352-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized...
A 0.4352-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized potassium hydroxide. The equivalence point in the titration is reached after the addition of 31.14 mL of 0.1833 M potassium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid. _____ g/mol
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
A sample of sodium carbonate (Na2CO3 (s), 105.99 g/mol) with a mass of 0.3531 g is...
A sample of sodium carbonate (Na2CO3 (s), 105.99 g/mol) with a mass of 0.3531 g is titrated with 0.042 L HCl (aq). Calculate the molarity of the HCl solution.
1.639 g of an unknown diprotic acis are used to make a 100.00 mL solutiob. Then...
1.639 g of an unknown diprotic acis are used to make a 100.00 mL
solutiob. Then 25.00 mL of this solution is trasferred to an
Erlenmeyer flask and is titrated with 0.1008 M NaOH. The titration
endpoint is reaxhed after 0.00432 mol of NaOH is added using the
burette. What is the molar mass of the diprotic acid? Provide your
answer to the correct nuber of significat figures
1.639 g of an unknown diprotic acid are used to make a...
25.247 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is aluted...
25.247 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is aluted with 72.054 g of water. A 11.243 g aliquot of this solution is then titrated with 0.1076 M HCI. It required 32.33 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste. Number wt% NH,-
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to...
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to phenolphthalein endpoint using 45.34 ml NaOH of unknown concentration. The formula weight of pure KHP is 204.22g/mol. Write the chemical equation for the neutralization reaction, indicate the color change of the indicator at the endpoint, and calculate molarity of the NaOH solution. Show your work. 1. Chemical equation ------------- 2. Endpoint color change ---- 3. NaOH molarity --------- Determine percent purity of impure KHP...
1 Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000443 mol...
1 Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000443 mol KIO30.0000443 mol KIO3 were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 17.80 mL17.80 mL. How many moles of Na2S2O3 did this require? 2. How many moles are present in a 25.00 mL sample of 0.076 M acetate? 3. A 25.00 mL solution containing 0.035 M sodium acetate is titrated with a 0.098 M solution of HCl. How many...
1. A volume of ___ mL of 0.100 M NaOH(aq) is required to titrate 0.500 g...
1. A volume of ___ mL of 0.100 M NaOH(aq) is required to titrate 0.500 g of potassium hydrogen phthalate (often abbreviated KHP) to the endpoint. 2. A 0.5741 g sample of a monoprotic acid was titrated with 0.1008 M NaOH(aq). If 37.89 mL of sodium hydroxide solution were required for the titration, the molar mass of the monoprotic acid is ___ g/mol.
Sodium carbonate, Na2CO3, reacts with hydrochloric acid, HCl, to produce sodium chloride, carbon dioxide and water....
Sodium carbonate, Na2CO3, reacts with hydrochloric acid, HCl, to produce sodium chloride, carbon dioxide and water. Refer to slide 7.18 for a summary of formulae relevant to the calculations below. 2HCl(aq) + Na.CO3(aq) + NaCl(aq) + H2O(l) + CO2(g) 1. Use this reaction to explain what is meant by the terms "acid", "conjugate base" and "salt" 2. Balance the equation for this reaction. 3. A solution was prepared by dissolving 5.00 g of Na2CO3 in water and adding water to...
25mL of an unknown sodium carbonate and sodium hydroxide mixture
reacted with 10mL of .5M SrCl2 is titrated with 1M HCl
Using the following endpoints determine (a) the number of moles
of NaOH and (b) the number of moles of Na2CO3. (Show work)
Endpoint 1: 13.2mL HCl used
Endpoint 2: 12.9mL HCl used
To the first endpoint: (1) HCI(aq) + NaOH (aq) NaCl(aq) + H20(0) Between the first and second endpoints: (2) 2 HCl(aq) + SrC03(s)SrCl2(aq) + H20() + CO2(aq)...
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
1.639 g of an unknown diprotic acis are used to make a 100.00 mL
solutiob. Then 25.00 mL of this solution is trasferred to an
Erlenmeyer flask and is titrated with 0.1008 M NaOH. The titration
endpoint is reaxhed after 0.00432 mol of NaOH is added using the
burette. What is the molar mass of the diprotic acid? Provide your
answer to the correct nuber of significat figures
1.639 g of an unknown diprotic acid are used to make a...
25.247 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is aluted with 72.054 g of water. A 11.243 g aliquot of this solution is then titrated with 0.1076 M HCI. It required 32.33 mL of the HCl solution to reach the methyl red endpoint. Calculate the weight percent NH3 in the aqueous waste. Number wt% NH,-
Standardization of NaOH solution experiment: A 0.75 g sample of pure acid KHP was titrated to phenolphthalein endpoint using 45.34 ml NaOH of unknown concentration. The formula weight of pure KHP is 204.22g/mol. Write the chemical equation for the neutralization reaction, indicate the color change of the indicator at the endpoint, and calculate molarity of the NaOH solution. Show your work. 1. Chemical equation ------------- 2. Endpoint color change ---- 3. NaOH molarity --------- Determine percent purity of impure KHP...
Sodium carbonate, Na2CO3, reacts with hydrochloric acid, HCl, to produce sodium chloride, carbon dioxide and water. Refer to slide 7.18 for a summary of formulae relevant to the calculations below. 2HCl(aq) + Na.CO3(aq) + NaCl(aq) + H2O(l) + CO2(g) 1. Use this reaction to explain what is meant by the terms "acid", "conjugate base" and "salt" 2. Balance the equation for this reaction. 3. A solution was prepared by dissolving 5.00 g of Na2CO3 in water and adding water to...
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