World News Headlines

Coverage of breaking stories

When the reaction H3PO4(aq)+Ca(OH)2(aq)→ occurs, what is the formula for the salt formed?

source : yahoo.com

When the reaction H3PO4(aq)+Ca(OH)2(aq)→ occurs, what is the formula for the salt formed?

H3PO4(aq)+Ca(OH)2(aq)→ ?

First step is to find what the products would be. Since this seems to be a double displacement, you get: H3PO4(aq)+Ca(OH)2(aq)→ H2O(L)+Ca3(PO4)2(s)

You know the products because H has a charge of +1, so PO4 must have a charge of -3, and since OH has a charge of -1, Ca must be +2. Then make each compound have a net charge of 0. H20 is a liquid since aq solutions have liquid water. Ca3(PO4)2 is a solid, use the solubility rules.

Lastly, balance the equation: 2H3PO4(aq)+3Ca(OH)2(aq)→ 6H2O(L)+Ca3(PO4)2(s)

So the salt formed is Ca3(PO4)2

When the reaction H3PO4+Ca(OH)2 occurs, what is the

When the reaction H3PO4+Ca(OH)2 occurs, what is the – When the reaction H3PO4+Ca(OH)2 occurs, what is the formula for the salt formed? Express your answer as a chemical formula. Update: I have to use subscripts to represent the number of each type of atom or ion in a molecule. I don't need the equation. I just need the formula.When the following reaction occurs:H3PO4 (aq) + Ca (OH)2 (aq) →What is the formula for the salt formed? Express your answer as a chemical formula.Reactions in water solution can be classified based on the driving force that converts reactants to product.When the reaction H3PO4 (aq) + Ca (OH)2 (aq) → occurs, what is the formula for the salt formed? A student placed 16.5 g of glucose (C6H1206) in a volumetric flask, added enough water to dissolve the glucose by swirling, then carefully added additional water until the 100. mL mark on the neck of the flask was reached.

Answer: Part B. When the following reactio… | Clutch Prep – What is the total ionic equation of this: 3CaCl2(aq) + 2K3PO4(aq) → Ca3(PO4)2(s) + 6KCl(aq) Shw all physical states of the reactants and products Chemistry Phosphoric acid reacts with magnesium hydroxide to produce magnesium phosphate and water via the following reaction:H3PO4 + Mg(OH)2 —–> Mg3(PO4)2 + H2O.Balance the equation, then enterFirst you find the products of the reaction. You don't need to balance it to find the chemical formula of the salt. H3PO4(aq)+Ca(OH)2(aq)→ H (OH) + Ca(PO4) I know the first one is water so the salt is the second compound. Then you find the charges of the components of the compound.. The charge of Ca is 2. The charge of PO4 is 3. Answer: Ca3(PO4)2For each reaction, identify the precipitate or lack thereof.2NaCI(aq) + Ba(OH)2 (aq) → BaCI2 + 2NaOHa) BaCI2b) NaOHc) no precipitate Q. Complete and balance each of the following equations for acid-base reactions.

Answer: Part B. When the following reactio... | Clutch Prep

Solved: When The Reaction H3PO4(aq) + Ca(OH)2(aq) → Occurs – How to solve: When the reaction H3PO4(aq) + Ca(OH)2(aq) occurs, what is the formula for the salt formed? By signing up, you'll get thousands of…Ca(OH)2 NH3. An acid is a covalently bonded substance that nonetheless produces _____when dissolved in water. This occurs because the acid molecules contains a(n) _____ covalent bond between H and another atom X (such as the bond in H-Cl). H3PO4 (aq) A(n) _____ acid or base will dissociate completely in water, whereas a(n) _____acid or baseExample \(\PageIndex{1}\): Neutralizing Nitric Acid. Nitric acid (HNO 3 (aq)) can be neutralized by calcium hydroxide (Ca(OH) 2 (aq)). Write a balanced chemical equation for the reaction between these two compounds and identify the salt that it produces.

(PDF) CHAPTER 1 CHEMISTRY: THE STUDY OF CHANGE Problem
Chemistry Archive | April 11, 2017 | Chegg.com

How to Write Dissociation Equations of Strong Electrolytes – TUTOR HOTLINE – Hey you're on the tutor hotline with Melissa Maribel how can I help you? Hi Melissa, it's Michele, can you help me with this question on writing dissociation equations for strong electrolytes? Of course, let's go over that.
So we're writing dissociation equations for strong electrolytes But let's go over what a strong electrolyte is So with this strong electrolyte which of course these are all strong electrolytes they completely dissociate and what dissociation refers to is just breaking apart into ions. So when a compound like let's say something like this, breaks apart or dissociates it completely breaks apart into its ions its really similar to net ionic equations so a type of strong electrolyte is a strong acid or a salt. And you'll notice that all of these are types of ionic compounds. A strong acid is something like HCl, so in this case what would happen, since this completely dissociates it would break apart into its separate ions which is Hydrogen plus or H+ and then chlorine with it's charge so -1 charge. Same thing goes for something like this strong acid, so nitric acid. Well I have hydrogen so it's going to be H+. I have that nitrate ion So that's going to be NO3 with a -1 charge And then if I were to let's say have something that is a salt, salt of course are ionic compounds if you remember. Ionic compounds consist of a metal and a nonmetal. The metal is positively charged and the nonmetal is negatively charged. And then of course the nonmetal could also be replaced with a polyatomic ion, which we see here with NO3 and same thing here with NO3. So for this first one this is a salt we have NaCl, I separate this apart to have it be NA+, because that's the charge of sodium and then Cl- I'll do the same exact thing here for this other salt where we have calcium and calcium's charge is a 2+ charge. And then nitrate has a -1 charge but the difference here is this subscript There are two nitrates so I have to indicate that there are also two NO3's in this equation and that's what makes it balanced. So this 3 subscript is part of nitrate already, right knowing your polyatomic ions is essential for these types of questions, and just Chemistry all together, where I know NO3 is nitrate, that doesn't mean that there's 3 NO's this NO3 is all together but this 2 subscript on the outside of the parentheses tells me that there are 2 nitrates Now that we understand how to break everything apart and what a strong electrolyte is, let's start off with part A. Ok, so the first thing with part A, what I'm going to do is just identify my metal and my nonmetal and them the charges for each So this is the metal that we have, cobalt it has a 3+ charge. If you didn't know what the charge was for cobalt that's ok, we could actually figure it out by just looking at this formula This Chemical formula Chlorine has a -1 charge The fact that there's a 3 subscript means that cobalt's charge must have been a 3+ So this 3 kinda goes back and it tells me that cobalt is a 3+ charge I know that this subscript also tells me that there are 3 chlorines So there's 3 chlorines and chlorine has a -1 charge How I'm going to write this dissociation equation .

pH of ionic compounds – – [Instructor] What happens
when you dissolve salt in water? Well as we talked about, for
example, sodium chloride, so sodium chloride when
in aqueous environment, we know that this will be converted to a sodium cation and a chloride anion.
So when this ionic compound
is surrounded by water, then the water molecules
can surround sodium through ion dipole interactions and surround chloride by
ion dipole interactions. And we end up with a
solution of sodium cations and chloride anions that are
fairly distinct from each other and they have the ability to undergo reactions by themselves if they can. And that idea that each of these two ions are now available to
react with other things is kind of the basis of
why some ionic compounds, when dissolved in water, will create an acidic or a basic solution. Let's take for example sodium fluoride instead of sodium chloride. So sodium fluoride is also
nice and soluble in water and when it dissolves in water we create a sodium cation and a fluoride anion. So the only difference in the products between these two
reactions is the presence of a chloride anion versus the
presence of a fluoride anion. And this is a really important difference because chloride is the conjugate
base of hydrochloric acid. We know that if we have hydrochloric acid reacting with water under an
acid dissociation reaction, we know hydrochloric acid's a strong acid so we completely convert into
chloride and to hydronium. So chloride is the conjugate
base of a strong acid meaning this reaction, chloride
will not react with water to be converted back over
here, this does not happen. So chloride does not undergo
a base dissociation reaction to produce hydrochloric acid because hydrochloric acid is a strong acid and this, the products are a
strong acid and a strong base and they would completely
revert back to reactants. So this reaction does not happen. Chloride is not able to serve as a base and react with water. Fluoride however is, so
fluoride is a weak base and when it reacts with water it undergoes a base dissociation reaction to produce HF, a weak acid, and hydroxide. Consequently, if we dissolve
sodium fluoride in water the fluoride that gets produced will react with water and make hydroxide. So when sodium fluoride
gets dissolved in water, we produce a weak base
which makes some hydroxide. So a solution of sodium fluoride will absolutely have a basic pH because in this compound is a weak base. Another example is, let's say
we have ammonium chloride. So ammonium chloride is
readily soluble in water so it will dissolve to make an ammonium cation and a chloride anion. As we just said, chloride is the conjugate base of a strong acid so it will not participate
in acid base chemistry. But ammonium will, ammonium is a weak acid which will react with water
to produce the ammonia, ammonia and in this case hydronium. So when ammonium chloride
is dissolved in water there's some hydronium that's produced so this will create an acidic solution. The big punch line here is that if the ionic compound contains a weak acid, then the solution will be acidic. If the ionic compound dissolves in water and contains a weak base then
the solution will be basic. How about this situation, so let's imagine dissolving sodium bicarbonate in water. This is nice and soluble
and when it dissolves we produce a sodium cation and
a hydrogen carbonate anion. Well bicarbonate is one of
these amphiprotic molecules. This is something you should've learned about in your reading. So amphiprotic means that
it can be an acid or a base. So it has the ability to
react with water and accept a proton or react with
water and donate a proton. So there are two possible reactions that bicarbonate can undergo. So it can react with
water to produce hydroxide in which case we generate carbonic acid. Or it can react with water and
an acid dissociation reaction and produce hydronium and its
conjugate base, carbonate. So these are two possible reactions that the bicarbonate ion
can undergo with water. Acid dissociation or base dissociation. So the question is which of
these will produce more product? Because if the base dissociation reaction has a larger equilibrium constant than more hydroxide will be produced. But if the acid dissociation reaction has a larger equilibrium constant then more hydronium will be produced. So the trick to this is to look up the acid dissociation constant
for the two reactions here and compare them, right so we need an equilibrium constant for
each of these two reactions. So let's refer to our table of pKa values. And I'll note that it's
a table of pKa values meaning we're only gonna find the values for acid dissociation reactions. So we will find this
first reaction directly but we're gonna need to figure out the pKb for the base dissociation reaction. So looking at this table here we find hydrogen carbonate, we
see bicarbonate here. It has pKa of 10.33 so
that acid dissociation reaction has a pKa of 10.33 or the Ka will be 10 to the negative 10.33. Let's compare this to
the equilibrium constant for the base dissociation reaction. Our process here is we wanna
find the conjugate acid of bicarbonate which is carbonic acid. So we have carbonic acid here. This is the pKa so the pKb is gonna be 14 minus this, so 7.65. So bicarbonate has a pKb of 7.65 so the equilibrium constant
is 10 to the negative 7.65. So this is our base dissociation constant. This is our acid dissociation constant. And since this value is larger. Since the kB value is larger this means bicarbonate is a better
base than it is an acid. So it's a better base than it is an acid so this reaction has the
larger equilibrium constant meaning the concentration
of hydroxide we produce will be larger than the
concentration of hydronium. So when you dissolve sodium
bicarbonate in water, we'll create a basic solution,
not an acidic solution because bicarbonate is a
better base than it is an acid. .

What is Neutralization? | HCl + NaOH | H2SO4 + NaOH – Dr K – In this video, we're going to answer the
following questions on neutralization.
Neutralization is a chemical reaction
that involves Arrhenius acid and base. Together they react to form salt and
water. Recall that Arrhenius acid can be represented as HA while Arrhenius base
is BOH. What happens in a neutralization equation is that the H
from acid and OH from the base will combine and they will form water, which
is H2O. Whereas the A from acid and B from base will combine to form salt, so,
the formula of salt is basically made out of the cation from the base and the
anion of the acid. That's pretty simple, right? So why is it that some people
struggle to write neutralization equations correctly? The reason lies in
the charges of A and B ions. Let's start by looking at simple neutralization
reaction between HCl and NaOH. When added to water, HCl will form H+ and Cl- and NaOH will form Na+ and OH-. Refer to the Arrhenius acid-base
theory video if you need more information on how to get the ions from
acid and base. The salt that is formed is made of Na+ and Cl-. We're basically just
forming ionic compound here so we just need to make sure that the charges are
balanced and a simple method of doing that is to do the crossover method. I'll
link the video if you need a refresher on writing the formula for ionic
compound, so, what we get when Na+ and Cl- get together is NaCl.
That's the formula of salt. It's pretty straightforward since we're dealing with
the same number of charges positive 1 and negative 1. What happens if we have
different number of charges for A and B ions? We'll take a look at the neutralization between H2SO4 and NaOH. NaOH formed Na+ and OH- and H2SO4 forms 2 H+ and SO4 2- ions. We have 2 H+ because
there are 2 hydrogens in the sulfuric acid formula. Sulphate ion, SO4 2-,
has a charge of negative 2 but let's just say we have no idea what's the
charge. Either it's not given to us or we have forgotten. How can we figure it out?
Well, remember how we can use the crossover method to write the formula of
ionic compound? All we have to do is work backwards. We were given the formula H2SO4. It's formed from H+ and SO4 something negative charge. Since we don't know we'll just use question mark to represent the charge number. We get the H2SO4 formula from crossover method like this. The charge on H+ is 1 so we
cross 1 over to SO4 and we get 1. As for the charge on SO4 which we don't know,
it's a question mark, we cross it over to H and we see a 2 there. That means the charge for SO4 is 2-. That's how we can figure out the charge of sulphate ion if it's
not given or we can't remember. Now that we've figure out the charge of sulphate ion,
we can continue with our neutralization equation. To form the salt we will need
2 Na+ ions for our SO4 2- ion. Just cross over Na+ with SO4 2-
and we will get the formula of salt as Na2SO4. Since we needed 2 Na+, that means we need 2 NaOH and in order to balance the equation as a
result we will produce 2 H2O. Therefore, our balanced neutralization equation will
be H2SO4 + 2 NaOH giving us Na2SO4 and 2 H2O. The key
to writing neutralization equation correctly is to figure out the right
formula for the salt and then to balance the entire equation. Do you want to try
writing a neutralization equation on your own?
How about using H3PO4 for acid and Mg(OH)2 for base? I'll place the answer in the
description box below. Let me know in the comments if you would like me to create
a video explaining how to write this neutralization equation. Hope you find the video helpful. Do subscribe and thanks for watching! .