Questions LLC
Login
or
Sign Up
Ask a New Question
Science
Chemistry
imagine that you have a 100 ml of HCl, after adding 50 ml of 1M NaOH, how many moles of OH did you add
1 answer
See your post above.
You can
ask a new question
or
answer this question
.
Similar Questions
imagine that you have a 100 ml of HCl, after adding 50 ml of 1M NaOH, how many moles of OH did you add
Top answer:
mols added = M x L = ?
Read more.
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70.
You have in front of you * 100 mL
Top answer:
To calculate the required amount of HCl needed to achieve the desired pH, we need to consider the
Read more.
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70.
You have in front of you * 100 mL
Top answer:
Start with 100 mL HCl, left with 83.0 means you have added 17.0 mL HCl to the beaker. Start with 100
Read more.
Given 20 mL NaOH; 0.1 M, add 0.05 M HCl, 10 mL at a time.
What is the pH initially of NaOH? What is the pH after adding 10 mL
Top answer:
This is the equivalent of an afternoon's work. What do you not understand about this and I can help
Read more.
Determine the pH during the titration of 40ml HCl (Ka= 1.3×10^-3) by 0.1M of NaOH ?
A) before the addition of any NaOH B) after
Top answer:
It's difficult
Read more.
Imagine that you are in chemistry lab and need to make 1.00 of a solution with a pH of 2.50.
You have in front of you 100 of
Top answer:
pH=log(H) 2=log H H=1E-2=.01M HCl net must be .01moles. You have .009*7E-2 moles or .009*.063 moles
Read more.
So I did a titration lab at school with NaOH and HCl. i have to find:
- volume used, NaOH - Moles of NaOH - Moles of HCl -Volume
Top answer:
Volume used NaOH: 35.8 mL (I subtracted 50 mL from 14.20 mL.. Am I doing this right??) <b> You did
Read more.
The titration of HCl with NaOH is represented by the equation
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) What volume of 0.100 M HCl
Top answer:
Any volume can titrate an acid with a base; you probably mean titrate to the equivalence point. For
Read more.
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
Top answer:
First, determine the M of the HCl. That will be 25*0.2/20 = 0.25M Where is the equivalence point.
Read more.
HCl is a strong acid and ionizes 100%.
NaOH is a strong base and ionizes 100%. We have no way of knowing the pH of HCl + H2O
Top answer:
To determine the pH of the final solutions, we need to consider the properties of the acids and
Read more.
Related Questions
An unbuffered solution contaning 0.000018 M HCl .Calculate PH after adding 1 mL of 0.1 M NaOH to 100 mL of solution.
A precipitate of copper(II) hydroxide is formed in a reaction. What change will help to dissolve the copper(II) hydroxide?
Cu^2+(
1.What mass of NaOH(s) must be added to 300 mL of HCl 0.25 M in order to completely neutralize this acid?
2.During a lab, you mix
21. Classify the following solutions in order of increasing pH:
a. 0.01 M NaOH b. pure water c. 0.10 M HCl d. 0.05 M NaOH e.
What is the molarity of HCL if it takes 16.5 mL of 0.100 M NaOH to titrate 10.0 mL of HCl?
HCl + NaOH -> H2O + NaCl molarity =
HCl is a corrosive colourless gas that dissolves readily in water.
Aqueous HCL reacts with NaOH to form water and NaCl. In a
If it requires 30.0 milliliters of 1.2 molar HCl to neutralize 20.0 milliliters of NaOH, what is the concentration of the NaOH
What volume of .100 M NaOH will react completely with 21.00 mL of .500 M HCl?
Vb*ConcBase= Vacid*ConcAcid Solve for Vb. 21.00 mL
You are given solutions of HCl and NaOH and must determine their concentrations. You use 38 mL of NaOH to titrate 100 mL of HCl
Product of this reasction?
1. Ag(NH3)2Cl + HCl? 2. AgOH + NaOH? 3. PbCl2 + HCl? 4. Pb(OH)2 + NaOH? 5. PbSO4 + (CH3COO)NH4? 6.
