An acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.
Their importance becomes apparent in analyzing acid–base reactions for gaseous or liquid species, or when acid or base character may be somewhat less apparent. The first of these concepts was provided by the French chemist Antoine Lavoisier, around 1776.
It is important to think of the acid-base reaction models as theories that complement each other. For example, the current Lewis model has the broadest definition of what an acid and base are, with the Brønsted-Lowry theory being a subset of what acids and bases are, and the Arrhenius theory being the most restrictive.
Homework Statement
Calculate the pH of the following solutions: (caution: these are hydrolysis reactions)
a. an 0.30 M solution of NaF
Homework Equations
I think by hydrolysis reactions they mean that each of the given compounds is combined with $H_2O$.
Then for
a) NaF + HF <-->...
Homework Statement
Calculate the pH of a 0.20 M solution of iodic acid ##(HIO_3)##. ##K_a## for iodic acid is 0.17
Homework Equations
##K_a = \frac{[H^+][IO_3^-]}{[HIO_3]}##
The Attempt at a Solution
##[HIO_3] = 0.20## M.
The concentration of ##[H^+]## and ##[IO_3^-]## should be the same...
Hi everyone. I was testing the pH of water that had alka seltzer placed in it. I used Bromothymol blue indicator to see the pH. The color changed to yellow, which suggests that the water was now acidic. I assume this is because of the CO2 bubbles that form which can acidify the H2O. Am I...
I tried looking for my unknown (209.70 g/mol) online and couldn't find it. The closest I found were H4O7V2(217.907 g/mol) and HCl2I(198.819 g/mol), but I know I am correct to a 2.7% accuracy. What other lists can I use to solve this?
Hi
I am new to the concept of neutralization.
My teacher told me that acids do not react with neutral salts.
I want to know why not. If both are dissolved in water and both completely dissociate, why can't the ions of acid and salt exchange and perform a double displacement reaction. Moreover I...
I was thinking of a hypothetical waste system that uses nanotechnology to its advantage.
At the individual level, waste just passes through into pipes when flushed like it normally does.
But once it reaches the water treatment plant there is an initial filter to catch solid waste(in other...
Homework Statement
To unclog a drain you add 26g of sodium hydroxide to 150mL of water. Calculate the pH and pOH for the solution you prepared. Can someone tell me if I'm doing it right.
Homework EquationsThe Attempt at a Solution
n = m/M
n = 26/40
n = 0.65mol for 0.15L
Does this mean that I...
Do pH and pKa refer to the same concept? The same question for pOH and pKb also.
What does kWh actually mean. In have read that it is the ionic product and is the product of [H+] and [OH-] but what does it indicate. Does it have any full form?
Since Acetic Acid is a weak acid, it has a low Ka which means that the forward reaction is not favored as much as the reverse reaction. However, the Kb is even lower than the Ka...how is this possible? Shouldn't the Kb be higher to indicate that the reverse reaction is favored?
Homework Statement
Student mix four reagents together, thinking the solutions will neutralize each other. The solutions mixed together are 50.0mL of .1 M HCl, 100mL of .2 M of HNO3, 500mL of .01 M CaOH, 200mL of .1 M RbOH. Did the acids and bases exactly neutralize each other? If not, calculate...
I'm having a lot of trouble predicting which compounds would be extracted into which layer (organic vs. aqueous) using acids and bases.
Using the solvents dichloromethane (which would form the organic layer) and sodium hydroxide (would form the aqueous layer along with water), I am asked to...
Homework Statement
In which one of the following solutions is silver chloride the most soluble?
A) 0.181 M HCl B) 0.0176 M NH3 C) 0.744 M LiNO3 D) pure water E) 0.181 M NaCl
Homework Equations
the Ksp expression for the dissolution of AgCl is:
Ksp = [Ag+][Cl-]The Attempt at a Solution...
Homework Statement
I found this problem online for extra practice for my AP Chem class.
https://www.quia.com/files/quia/users/jpugteach/APChem/AP-Chem-Chapter-19-Graphs.pdf
The problem in question is number 4.
I do not understand how to solve it and why the answer D is correct.
Homework...
Homework Statement
Methyl red has the following structure [not listed here on this post]
Ka = 5.0 * 10 E -5
It undergoes a color change from red to yellow as a solution gets more basic.
Calculate an approximate pH range for which the methyl red is useful.
What is the color change and the...
Homework Statement [/B]
NH3(aq) is a weak base with Kb = 1.8*10-5, Calculate [OH-] in a solution that is made by mixing togeather 500ml of 0.20M NH3(aq) and 500ml of 0.20M NH4CL(aq), what is the value of Ph?Homework Equations
Henderson Hasselbalch: ph = Pka + log([conj.base/acid])
As well as...
Hey all!
I have a silly doubt
In acids and bases
As you guys know
The concentration of H+ ions
For a weak acid
Which does not undergo
Complete dissociation
Is given by mod H+=square root of Ka times C
Where C is the initial concentration
Of the acid
And k is the ionization constant
In the same...
Hi guys, my name is ferdinand. I'm curious about HSAB, especially to predict where the reaction goes.
Exp: HI + NaF >>> HF + NaI
H is hard acid
I IS soft base
Na is hard acid
F is hard base, and
HF Is hard.hard
NaI Is hard soft.
The reaction will goes to right or left? And why?
And since hard...
what theories out of the major two ( Bronsted-Lowry Theory of acids and bases and The Lewis Theory of acids and bases) should we use in common problems, and which one is more reliable ?
Homework Statement
the question asks to determine if the equilibrium is greater, equal or less than 1. one of the equation is the following:
[CuI4]2- (aq) + [CuCl4]3- (aq) ↔ [CuCl4]2-(aq) + [CuI4]3- (aq)
Homework Equations
The Attempt at a Solution
the solution given was...
Homework Statement
Assuming stomach acid is 0.1 M HCl(aq), what volume of stomach acid can be neutralized by one antacid tablet?
We have the titration curve we got with .5M HCl titrating a tablet dissolved in 100ml distilled water
Homework Equations
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The Attempt at a Solution
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Homework Statement
1.5000 g of diprotic weak acid H2A was dissolved in 100.00 mL volumetric flask.
25.00 mL aliqouts of this solution was titrated with a monoprotic strong base NaOH (0.08000 M). The titre volume of NaOH was 40.00 mL. Calculate the molecular weight of H2A.
Homework...
Homework Statement
Hi. I'm reaady to panic right now so if anyone could please take the time to answer my question I would HUGELY appreciate it! I seriously need to get this done soon as I also have a test tomorrow and i just want to cry because I'm getting nowhere...
We did a lab...
Homework Statement
after titrating sodium hydroxide with hydrofluoric acid, a chemist determined that the reaction had formed an aqueous solution of 0.020 mol/l sodium fluoride. determine ph of the solution
Homework Equations
The Attempt at a Solution
Ka of HF= 6.3X10^-4
NaOH +...
Hi. In class, i am required to perform a titration where i am given a solution of sodium carbonate and a solution of hydrochloric acid of known concentration. I am to use the acid to calculate the percentage purity of the sodium carbonate.
Im not really sure how to go about doing this. The...
Homework Statement
Do not understand the question.
2. My Lab Results
Topic : Volumetric analysis - Acid base
purpose : To determine the exact concentration of a mineral acid, HXO4, and to determine the relative atomic mass of the element X.
Materials : KA1 is a mineral acid, HXO4...
Hello everybody, I'm having difficulty understanding the rationalization behind the strengths of Bronstend Lowry acids and bases and my textbook isn't too helpful. Can someone please expalin to me: (1) What exactly is effective negative charge density? (2) how does electronegativiy correspond to...
Homework Statement
Given H2SO4 + 2LiOH --> Li2SO4 + 2H2O, how many mL of a 0.700-M solution of KOH are needed to react with 235 mL of a 0.350-M H2SO4 solution?
The Attempt at a Solution
Really, I have none. My problem is that I don't understand what the question is asking. I could...
Homework Statement
You dissolve an unknown quantity of weak acid HA into 50 mL of water. It only takes 1 mL of 5 M NaOH to completely neutralize the acid. The Ka of the acid is 3.2 x10^-4. What is the pH at the endpoint?Homework Equations
Ka * Kb = Kw
pH + pOH = 14
p(of whatever) = -log(of...
Homework Statement
A vessel contains 500mL of .1 molar H2S solution. For H2S Ka1 = 1 x 10^-7
Ka2 = 1.3 x 10^-13.
What will the pH be when 800mL of .1molar NaOH has been added.
Homework Equations
ph = -log([H])
ph = pka + log(B/A)The Attempt at a Solution
This is how I started, I found the...
I tried looking for this online, but didn't really find anything can someone help me out I need an example of a naturally- occurring acid-base buffering system in an organism
I have a question concering acid base reactions. All strong acid-strong base reactions produce a water soluble salt and water with the exception of what? I need to know that along with the formula unit, total ionic and net ionic equation. Please any help would be appreciated. Thank you
Hi.
I am having trouble with acid-base titration excercises. 0.02 L butanoic acid @ 0.1 M is titrated with 0.01 L NaOH solution @ 0.1 M. The Ka of butanoic acid is 1.54X10^-5. Find the pH. The answer is 4.81. I know how to find the pH when no NaOH is added, but I really don't see how the...
How many moles of H3O+ must be added to one liter of a solution to adjust the pH from 7.17 to 5.85?
Correct answer 1.34E-6 (1.34 * 10-6)
The correct answer is given, however I would like to know how to do this problem.
consider the titration of 50.0mL of 0.10 M methyl ammonia with 0.10 M HCl. Calculate the pH after
15mL of titrant= 11.05
25mL of titrant= 10.68
50mL of titrant= 8.98
60mL of titrant= ?
At 60 mL there is an excess of 1 mmol of HCl. At this point do I say that the pH is 1 (-log of 0.10)...
I have several questions.
1.)Supose [H+] is 100 times less than the ka for an acidic acid-base indicator (see Eq.2), and enough acid is added to the the solution to raise [H+] by a factor of 10,000. What value did the ration of the different colored forms of the indicator, [ln-]/[H ln], have...