Classify the aq solution of the following salts into acidic basic and neutral??

KCl,NH4NO3,Na2CO3,K2CO3

How to find it???

Pls reply fast Monday is my chemistry board exams!!

acidic - NH4NO3 (NH4OH is a weak base and HNO3 is a strong acid so overall salt is acidic salt)

Basic- Na2CO3 and  K2CO3 (NaOH and KOH both are strong base while H2CO3 is weak acid)

Neutral- KCl (Both KOH and HCl are strong base and base respt. so the salt is neutral)

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 Guidelines for writing names and formulas for compounds
Type of
compound General formula Examples General name Examples
Binary
covalent
Section 3.4
AaBb
N2O5
or CO2
(prefix unless mono)(name of first element in
formula) (prefix)(root of second element)ide
dinitrogen pentoxide
or carbon dioxide
Binary ionic
Section 3.5 MaAb
NaCl
or FeCl3
(name of metal) (root of nonmetal)ide
or (name of metal)(Roman ) (root of
nonmetal)ide
sodium chloride
or iron(III) chloride
Ionic with
polyatomic
ion(s)
Section 3.5
MaXb or (NH4)aXb
X = recognized
formula of
polyatomic ion
Li2HPO4
or CuSO4
or NH4Cl
or
(NH4)2SO4
(name of metal) (name of polyatomic ion)
or (name of metal)(Roman ) (name of
polyatomic ion) or ammonium (root of
nonmetal)ide
or ammonium (name of polyatomic ion)
lithium hydrogen
phosphate
or copper(II) sulfate
or ammonium chloride
or ammonium sulfate
Binary acid
Section 5.2 HX(aq) HCl(aq) hydro(root)ic acid hydrochloric acid
Oxyacid
Section 5.2 HaXbOc
HNO3
or H2SO4
or H3PO4
(root)ic acid
nitric acid
or sulfuric acid
or phosphoric acid
Notes: M = symbol of metal
A and B = symbols of nonmetals
X = some element other than H or O
a, b, & c indicate subscripts
 The significance of the numbers in the pH scale
54 Study Guide for An Introduction to Chemistry
To get a review of the most important topics in the chapter, fill in the blanks in the Key
Ideas section.
Work all of the selected problems at the end of the chapter, and check your answers with
the solutions provided in this chapter of the study guide.
Ask for help if you need it.
Web Resources
Internet: Acid Animation
Internet: Types of Substances
Internet: Chemical Nomenclature
Internet: Strong and Weak Bases
Internet: Identification of Strong and Weak Acids and Bases
Internet: Acid-Base Reaction
Internet: Glossary Quiz
Exercises Key
Exercise 5.1 - Formulas for Acids: Write the chemical formulas that correspond to the
names (Obj 12)
(a) hydrofluoric acid
This name has the form of a binary acid, hydro(root)ic acid, so its formula is
HF(aq).
(b) phosphoric acid
This name has the form of an oxyacid, (root)ic acid, so it contains hydrogen,
phosphorus, and oxygen. Phosphate is PO4
3, so phosphoric acid is H3PO4.
Exercise 5.2 - Naming Acids: Write the names that correspond to the chemical formulas
(Obj 12)
(a) HI(aq)
This is a binary acid, so its name has the form hydro(root)ic acid. HI(aq) is
hydriodic acid. (The “o” in hydro- is usually left off.)
(b) HC2H3O2.
The name of the oxyanion C2H3O2
– is acetate, so HC2H3O2 is acetic acid.
CH3CO2H and CH3COOH are also commonly used as formulas for acetic acid.
Exercise 5.3 - Formulas to Names: Write the names that correspond to the following
chemical formulas. (Obj 14)
a. AlF3 aluminum fluoride
b. PF3 phosphorus trifluoride
c. H3PO4 phosphoric acid
d. CaCO3 calcium carbonate
e. Ca(HSO4)2 calcium hydrogen sulfate
f. CuCl2 copper(II) chloride
g. NH4F ammonium fluoride
h. HCl(aq) hydrochloric acid
i. (NH4)3PO4 ammonium phosphate
Chapter 5 – Acids, Bases, and Acid-Base Reactions 55
Exercise 5.4 - Names to Formulas: Write the chemical formulas that correspond to the
following names. (Obj 14)
a. ammonium nitrate NH4NO3
b. acetic acid HC2H3O2
c. sodium hydrogen sulfate NaHSO4
d. potassium bromide KBr
e. magnesium hydrogen phosphate
MgHPO4
f. hydrofluoric acid HF(aq)
g. diphosphorus tetroxide P2O4
h. aluminum carbonate Al2(CO3)3
i. sulfuric acid H2SO4
Exercise 5.5 - Identification of Acids and Bases: Identify each of the following as an
Arrhenius strong acid, an Arrhenius weak acid, an Arrhenius strong base, or an Arrhenius weak
base. (Obj 18)
a. HNO3 strong acid
b. lithium hydroxide strong base
c. K2CO3 weak base
d. hydrofluoric acid weak acid
Exercise 5.6 - Neutralization Reactions: Write the complete equation for the
neutralization reactions that take place when the following water solutions are mixed. (If an acid
has more than one acidic hydrogen, assume that there is enough base to remove all of them.
Assume that there is enough acid to neutralize all of the basic hydroxide ions.) (Obj 24)
a. HCl(aq)  NaOH(aq)  H2O(l)  NaCl(aq)
b. HF(aq)  LiOH(aq)  H2O(l)  LiF(aq)
c. H3PO4(aq)  3LiOH(aq)  3H2O(l)  Li3PO4(aq)
d. Fe(OH)3(s)  3HNO3(aq)  Fe(NO3)3(aq)  3H2O(l)
Exercise 5.7 - Neutralization Reactions with Compounds Containing Carbonate:
Write the complete equation for the neutralization reaction that takes place when water solutions
of sodium carbonate, Na2CO3, and hydrobromic acid, HBr, are mixed.
(Obj 24)
Na2CO3(aq)  2HBr(aq)  2NaBr(aq)  H2O(l)  CO2(g)
Exercise 5.8 - Conjugate Acids: Write the formula for the conjugate acid of (a) NO2
–, (b)
HCO3
–, (c) H2O, and (d) PO4
3–. (Obj 27)
a. HNO2 b. H2CO3 c. H3O d. HPO4
2–
Exercise 5.9 - Conjugate Bases: Write the formula for the conjugate base of (a) H2C2O4,
(b) HBrO4, (c) NH3, and (d) H2PO4
–. (Obj 28)
a. HC2O4
– b. BrO4
– c. NH2
– d. HPO4
2–
Exercise 5.10 - Brønsted-Lowry Acids and Bases: Identify the Brønsted-Lowry acid and
base in each of the following equations. (Obj 31)
a. HNO2(aq)  NaBrO(aq)  HBrO(aq)  NaNO2(aq)
B/L acid B/L base
b. H2AsO4
–(aq)  HNO2(aq) H3AsO4(aq)  NO2
–(aq)
B/L base B/L acid
c. H2AsO4
–(aq)  2OH–(aq)  AsO4
3–(aq)  2H2O(l)
B/L acid B/L base
56 Study Guide for An Introduction to Chemistry
Review Questions Key
1. Define the following terms.
a. aqueous
Water solutions are called aqueous solutions.
b. spectator ion
Ions that are important for delivering other ions into solution to react, but do not
actively participate in the reaction themselves are called spectator ions.
c. double-displacement reaction
A chemical reaction that has the following form is called a double-displacement
reaction.
AB + CD  AD + CB
d. net ionic equation
A net ionic equation is a chemical equation for which the spectator ions have
been eliminated leaving only the substances actively involved in the reaction.
2. Write the name of the polyatomic ions represented by the formulas CO3
2– and HCO3
–.
a. CO3
2– carbonate b. HCO3
– hydrogen carbonate
3. Write the formulas for the polyatomic ions dihydrogen phosphate ion and acetate ion.
a. dihydrogen phosphate ion H2PO4
– b. acetate ion C2H3O2

4. Which of the following formulas represents an ionic compound?
a. MgCl2 ionic
b. PCl3 not ionic
c. KHSO4 ionic
d. Na2SO4 ionic
e. H2SO4 not ionic
5. Write the names that correspond to the formulas KBr, Cu(NO3)2, and (NH4)2HPO4.
a. KBr potassium bromide
b. Cu(NO3)2 copper(II) nitrate
c. (NH4)2HPO4 ammonium hydrogen
phosphate
6. Write the formulas that correspond to the names nickel(II) hydroxide, ammonium chloride,
and calcium hydrogen carbonate.
a. nickel(II) hydroxide Ni(OH)2
b. ammonium chloride NH4Cl
c. calcium hydrogen carbonate
Ca(HCO3)2
7. Predict whether each of the following is soluble or insoluble in water.
a. iron(III) hydroxide insoluble
b. barium sulfate insoluble
c. aluminum nitrate soluble
d. copper(II) chloride soluble
8. Describe the process by which the ionic compound sodium hydroxide dissolves in water.
When solid sodium hydroxide, NaOH, is added to water, all of the sodium ions, Na+, and
hydroxide ions, OH–, at the surface of the solid can be viewed as shifting back and forth
between moving out into the water and returning to the solid surface. Sometimes when an
ion moves out into the water, a water molecule collides with it, helping to break the ionic
bond, and pushing it out into the solution. Water molecules move into the gap between
the ion in solution and the solid and shield the ion from the attraction to the solid.
The ions are kept stable and held in solution by attractions between them and the polar
water molecules. The negatively charged oxygen ends of water molecules surround the
sodium ions, and the positively charged hydrogen ends of water molecules surround the
hydroxide ions. (See Figures 4.4 and 4.5 with OH– in the place of Cl–.)

 

hope it helps

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 But Heena didi pls explain in a simple way I cannot understand I'm feeling tensed!!

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