May 25, 2019, 03:25:45 PM
Forum Rules: Read This Before Posting

### Topic: Titrating Na2CO3 Solution with HCl  (Read 80454 times)

0 Members and 1 Guest are viewing this topic.

#### themann

• Guest
##### Titrating Na2CO3 Solution with HCl
« on: March 23, 2006, 05:16:18 AM »
Once again i am unsure. If i have 25mL of Na2CO3 0.1M solution How much HCl would i approximately need to add. Say as a ratio from 1 mole of HCL i get 1 +H ion will i get 1 -OH ion as a result or will i get 2 or more. It seems to my understanding that it would be a 1 to 1 ratio but once again i am unsure. If it was a 1 to 2 ratio it would mean that 50mL of HCL would be needed for every 25mL of Na2CO3 solution titrated.

#### cathy

• Guest
##### Re:Titrating Na2CO3 Solution with HCl
« Reply #1 on: March 23, 2006, 05:34:28 AM »
I think :::
Since Na2CO3+2HCl-->CO2+H2O+2NaCl
1 mole of NaCO3 reacts with 2 mole of HCl
no. of mole of Na2CO3=molarity * volume(in dm3)
=25*10-3mole
So that no. of mole of HCl= no. of mole of Na2CO3 * 2
=5*10-3
volume of HCl used = no. of mole of HCl / molarity of HCl
if you used 0.1M of HCl,
then  volume of HCl = 50mL
But I am not sure is this correct ^ ^"

#### cuongt

• Full Member
• Posts: 102
• Mole Snacks: +15/-22
• Gender:
• I'm a mole!
##### Re:Titrating Na2CO3 Solution with HCl
« Reply #2 on: March 23, 2006, 05:41:01 AM »
yep ratio is 1:2 so u would need 50mL of HCl for every 25mL of Na2CO3.

You are both rite.

#### AWK

• Retired Staff
• Sr. Member
• Posts: 6419
• Mole Snacks: +462/-79
• Gender:
##### Re:Titrating Na2CO3 Solution with HCl
« Reply #3 on: March 23, 2006, 05:42:01 AM »
Na2CO3 reacts with HCL in two steps

Na2CO3 = HCl = NaHCO3 + NaCl
NaHCO3 + HCl = H2O + CO2(g) + NaCl
For each step you need equimolar amount of HCl

If you use 0.1 M HCl then you need twice 25 ml od acid for 25 ml of 0.1 M Na2CO3.
AWK

#### Borek

• Mr. pH
• Administrator
• Deity Member
• Posts: 25010
• Mole Snacks: +1642/-395
• Gender:
• I am known to be occasionally wrong.
##### Re:Titrating Na2CO3 Solution with HCl
« Reply #4 on: March 23, 2006, 05:49:42 AM »
See titration curve. There are two endpoints, all depends on the indicator used (although first is way to flat for a good precision).
« Last Edit: March 23, 2006, 05:51:35 AM by Borek »
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info, pH-meter.info, PZWT_s1

#### themann

• Guest
##### Re:Titrating Na2CO3 Solution with HCl
« Reply #5 on: March 24, 2006, 07:13:10 PM »
ok great thanks guys. Beacause i am given 2 indicators methyl orange and phenylphthaline. The two endpoints show that the first would be detected by phenylphthaline and the second with methyl orange. so am i best off just using methyl orange to get a better precision. Does the CO2 pose a problem to the H20 which in essence might form HCO3? or something of the eqivalent?