Login
Remember
Register
Science Q&A Sarvan.Net
All Activity
Q&A
Questions
Hot!
Unanswered
Tags
Categories
Users
Ask a Question
About Us
XML Sitemap
Terms of Service
Ask a Question
What is the balanced chemical equation for the reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH) to produce sodium chloride (NaCl) and water (H2O)?
0
votes
82
views
asked
Feb 17
in
Chemical reactions
by
Candida6637
(
1.6k
points)
What is the balanced chemical equation for the reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH) to produce sodium chloride (NaCl) and water (H2O)?
Please
log in
or
register
to add a comment.
Please
log in
or
register
to answer this question.
1
Answer
0
votes
answered
Feb 17
by
KaraMcRae960
(
2.5k
points)
The balanced chemical equation for the reaction of hydrochloric acid HCl with sodium hydroxide NaOH to produce sodium chloride NaCl and water H2O is:HCl + NaOH NaCl + H2O
Please
log in
or
register
to add a comment.
Related questions
0
votes
1
answer
81
views
Consider the chemical reaction between sodium hydroxide (NaOH) and hydrochloric acid (HCl) to produce sodium chloride (NaCl) and water (H2O). Write a balanced chemical equation for this reaction and determine the mole ratio of NaOH and HCl required for complete reaction. If we start with 10 grams of NaOH and 20 grams of HCl, determine which is the limiting reagent, the amount of excess reagent left over, and the mass of NaCl and H2O produced.
asked
Feb 3
in
Inorganic Chemistry
by
DoloresLocke
(
1.7k
points)
0
votes
1
answer
78
views
What is the balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O)?
asked
Feb 17
in
Chemical reactions
by
Dylan31U6281
(
2.0k
points)
0
votes
1
answer
126
views
Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given that the reaction produces water and sodium chloride as products. The molar enthalpy of formation for water is -285.8 kJ/mol and for NaCl is -411.2 kJ/mol. The balanced chemical equation for the reaction is: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
asked
Feb 3
in
Chemical thermodynamics
by
SilviaTorpy5
(
2.1k
points)
0
votes
1
answer
130
views
Calculate the standard enthalpy change (in kJ/mol) for the reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O), given the following balanced chemical equation:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)Assume the reaction takes place under standard conditions (298 K and 1 atm pressure) and that all solutions have a concentration of 1.0 M. The standard enthalpies of formation for HCl (aq), NaOH (aq), NaCl (aq), and H2O (l) are -92.31 kJ/mol, -469.14 kJ/mol, -407.76 kJ/mol, and -285.83 kJ/mol, respectively.
asked
Feb 3
in
Chemical thermodynamics
by
JacquelynDos
(
1.7k
points)
0
votes
1
answer
80
views
What is the balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), and how many moles of sodium chloride (NaCl) will be produced when 50 mL of 0.1 M HCl is reacted with excess NaOH?
asked
Feb 17
in
Chemical reactions
by
Sylvia941924
(
1.9k
points)
37.4k
questions
37.2k
answers
2
comments
17.6k
users
Categories
All categories
Science
(12.0k)
Psychology
(10.5k)
Chemistry
(14.9k)
Organic Chemistry
(663)
Inorganic Chemistry
(568)
Physical Chemistry
(613)
Analytical Chemistry
(657)
BioChemistry
(719)
Polymer Chemistry
(720)
Medicinal Chemistry
(680)
Environmental Chemistry
(684)
ElectroChemistry
(379)
Computational Chemistry
(681)
Materials Chemistry
(641)
Surface Chemistry
(704)
Coordination Chemistry
(632)
Quantum Chemistry
(684)
ThermoChemistry
(573)
PhotoChemistry
(731)
Chemical kinetics
(639)
Chemical thermodynamics
(560)
Chemical equilibrium
(318)
Chemical bonding
(656)
Chemical reactions
(412)
Chemical synthesis
(532)
Chemical engineering
(614)
Chemical education
(836)
Welcome to Sarvan Science Q&A, where you can ask questions and receive answers from other members of the community.
...