Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Stoichiometry
Titration
By titration it is found that 76.3Ml of 0.178M of NaOH(aq) is needed to neutralize 25.00mL of HCL(aq). Calculate the concentration of the HCl solution.
1 answer
mL acid x M acid = mL base x M base
You can
ask a new question
or
answer this question
.
Similar Questions
In a silphuric acid (H2SO4)-Sodium Hydroxide (NaOH) acid-base titration, 17.3mL of 0.126M NaOH is needed to neutralize 25mL of
Top answer:
morality? Most H2SO4 solutions are not moral at all. Neither are NaOH solution. H2SO4 + 2NaOH ==>
Read more.
How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O
The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of
Top answer:
mols NaOH = M x L = ? mols HAc = mols NaOH (look at the coefficients in the balanced equation). M
Read more.
How to solve titration problem for HC2H3O2 + NaOH= NaC2H3O2 + H2O
The M of NaOH= 0.427 The volume of NaOH= 17.30mL 10.00mL of
Top answer:
mols NaOH = M x L = ? mols HC2H3O2 = the same (note the balanced equation and 1 mol NaOH reacts with
Read more.
What volume of 0.115 M M HClO 4 \rm HClO_4 solution is needed to neutralize 58.00mL mL of 8.75×10−2 M M NaOH \rm NaOH
Top answer:
Worked like the last one like this. HClO4 + NaOH ==> NaClO4 + H2O mols NaOH = M x L = ? mols HClO4 =
Read more.
By titration it is found that 66.1 mL of 0.125 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
Top answer:
mLNaOH x M NaOH = mL HCl x M HCl
Read more.
By titration it is found that 12.1 mL of 0.130 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
Top answer:
NaOH + HCl ==> NaCl + H2O mols NaOH = M x L = ? mols HCL = mols NaOH since 1 mol NaOH reacts with 1
Read more.
By titration it is found that 68.9 mL of 0.122 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
Top answer:
mL acid x M acid = mL NaOH x M NaOH.
Read more.
By titration it is found that 69.9 mL of 0.151 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
Top answer:
mL1 x M1 = mL2 x M2 This equation works because the mols HCl = mols NaOH.
Read more.
By titration it is found that 20.5 mL of 0.168 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
Top answer:
Aren't these the same problem? You didn't look to see your old post?
Read more.
By titration it is found that 20.5 mL of 0.168 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
Top answer:
HCl + NaOH ==> NaCl + H2O mols NaOH = M x L =? Using the coefficients in the balanced equation,
Read more.
Related Questions
The titration of 25.00ml of 0.1000m hypochlorous acid (3.5x10^-8) with 0.1500m NaOH.
(a). What is the pH before any acid is added
Which of the following solutions should be used when titrating a 25.00mL sample of CH3COOH that is approximately 0.1 M?
a.) 0.150
During an acid-base titration, 25 mL of NaOH 0.2 M were required to neutralize 20 mL of HCl.
Calculate the pH of the solution for
Determine the concentration of a NaOH solution if 27.80mL of NaOH is required to neutralize 10.00mL of a 1.00 M H2SO4 solution.
Consider the titration of 25.0mL of 0.10M HAc with 0.10M NaOH. That is, NaOH is added to HAc. (a)pH at the beginning of
calculate the molarity of acetic acid in a vinegar sample,knowing that 5.00ml of vinegar requires 43.50ml of 0.105 M NaOH to
In Chemistry: what is ph during the titration of 20.00ml of 0.1000m triethylamine (ch3ch2)3n (kb=5.2x 10-4) with 0.1000m HCL
Find the pH during the titration of a 20.00mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka=1.54 x10^-5), with the addition of 10
in a titration, 0.0400 mol of solid NaOH is required to neutralize 10.0 mL of H2SO4(aq). From these data, the [H2SO4] is:
1.3188g of antacid is weighed and mixed with 75.00mL of excess 0.1746M HCl. The excess acid required 27.20mL of 0.09767M of NaOH