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11 Dec 2019

A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.150 g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample?

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Reid WolffLv2
13 Dec 2019
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Related questions

Some quanity of Na2CO3 has been dissolved in water. You titrate the solution with 0.100 M HCl (aq) and determine that 40.00 mL of 0.100 M HCl (aq) is required to reach the end point of a titration. What mass of Na2CO3 was present in the sodium carbonate solution?

A 0.3147 g sample containing Na2CO3 was dissolved in 60 mL of distilled H2O and 2-3 drops of methyl orange were added to the mixture. The solution needed 38.73 mL of 0.1214 M HCl to reach the methyl orange end point. a.Calculate the number of millimoles of HCl needed to reach the methyl orange end point. b.How many millimoles of Na2CO3 reacted with the HCl?c.What is the mass(g) of Na2CO3 present in the sample?d.What is the %Na2CO3 present in the sample?please show your complete solution please:)

Please help with the last two parts!!

1.A 1.478 g sample of soda ash required 17.41 mL of 0.6714 MHCl to reach the second endpoint. Determine the % Na2CO3in the soda ash sample.

0.6714 M X 0.01741 L = 0.01169 mol HCl

0.01169 mol HCl X X = 0.6195 g Na2CO3

( 0.6195 g Na2CO3/ 1.478 g Na2CO3) X 100 = 41.91% Na2CO3

2.A particular soda ash sample contains 20.33% Na2CO3. How many mL of 0.4009 MHCl would be required to neutralize a 1.559 g of this soda ash sample?

3.Let’s suppose you didn’t follow the procedure and failed to quantitatively transfer the soda ash sample to the Erlenmeyer flask. How would this specifically affect your calculated percentage of Na2CO3?

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