Acid Base And Salt Worksheet Pdf

[Recaredo Latreche]

Substancesthat we use daily can be classified as acids, bases, and neutral substances. For example, lemon juice is acidic, and baking soda solution is basic and common salt is neutral. Lemon juice is acidic since lemon contains citric acid. Similarly, baking soda contains sodium bicarbonate which acts as a base. Sodium chloride is a salt formed by the neutralisation reaction between an acid and a base.

First, you need to memorize the strong acids and bases. This is key. It will not only allow you to identify the strong acids andbases, but it will help you figure out which ions are simply spectator ions.

Second, you should realize that history has played a role in naming compounds. Therefore there are some compounds we typically think of as acids and some compounds we think of bases. However, every acid has a conjugate base and every base a conjugate acid. So we really have two forms of each compound: one protonated (the acid) and one deprontonated (the base).

Names of acids are typically "something"-acid. As such they are readily identified. Weaks acids are the acids that arenot strong. Memorize the strong acids and you'll know everything else is weak. For example, the following are all weak acids:lactic acid, benzoic acid, oxalic acid, trichloroacetic acid, ...The chemical formula for the acids depends on the type of acid (hydroacid, oxoacid, or carboxylic acid).In particular you want to be able to recognize the carboxylic acid group that is found in many organic molecules. It is anoxygen double-bonded to a carbon with an OH group on the same carbon. This is denoted by RCOOH, where the R is a generic representation of therest of the molecule. For example, formic acid is HCOOH (R = H), acetic acid is CH3COOH (R = CH3).

These weak acids are all compounds that are "uncharged" in their protonated state.If we neutralize them with an strong base we will end up with a salt composed of a cation and an anion. The anion is theconjugate base of the acid. This is an important clue to the identity of the species. If the acidic compound is not chargedonce you remove H+ from the compound you will form an anion. Where there is an anion there is always a cation to balancethe charge. The cation will be a spectator. Thus the basic salts will be composed of a spectator ion like sodium, Na+, potassium,K+ or something like that and an anion that is the conjugate base of the acid. They can be identified as they are thesame compound as the weak acid but they are "missing" a H+. Thus F- is the conjugate base of HF. NaF is abasic salt. K(CH3COO), potassium acetate, is a basic salt that contains the acetate anion that is the deprotantatedform of acetic acid. Their names are also helpful in identification. The names of the anions often end in "ate". The benzoate ionis deprotonated benzoic acid. The formate ion is the conjugate base of formic acid.

Weak bases are typically compounds that are like substituted ammonia, NH3. In these compoundsthe H's have been replaced with something else (like a carbon chain). For example, methyl amine, is CH3NH2. OneH has been replaced with a CH3. There is a near endless list of such compounds. As a class, they are called "amines". Thus "something something" amine is identifiable as a weak base. What about their conjugate acids? Since the amines have no charge, if they accept a proton they will add H+. This means their conjugated acids will be positively charged and will formsalts with spectator anions. Therefore something like methylammonium chloride (CH3NH3)Cl can be identified as an acidic salt.

What about salts that combine a basic anion and an acidic cation? Consider for example, ammoniumfluoride (NH4F). Here the ammonium ion (NH4+) is an acid and the fluoride ion (F-) is a base. These "mixed" salts are best thought of simply as either acids or bases.

There are also compounds with more than one acidic proton (polyprotic species). These will form anions that can be both acids and bases. These species are called, amphiprotic. They can be identified as anions that still have acidic protons. For example, HCO3-. This is carbonic acid, H2CO3 that has lost one proton.It is both an acid and base. This will be covered more in detail with polyprotic acids.

Finally, there are a few exceptions to these ideas. First there are neutral salts, like NaCl. In this case, both the cation and the anion are the conjugate pair of a strong acidand strong base. As such, a solution of these ions will be neutral. If you have memorized the strong acids and strong bases, thesecan quickly be identified. Second, there are a number of insoluble hydroxides, like Al(OH)3 that are weak simply since they don't dissolve in water. They don't really have aconjugate acid. They are weak simply as a result of solubility.

You will learn how to identify acids and bases based on their chemical symbol and you will learn to predict where they might fall on the pH scale. You will also begin to realize the relative strength of these substances based on the nature of the elements that are involved. You will also learn how the nature of a liquid can help you understand if they are good conductors of electricity. The worksheets work on identifying acids and bases based on a number of different criteria and your understanding of ion transfer.

Identify whether the solutions listed below are acids or bases. Write the color expected for eachindicator (phenolphthalein, litmus dye) when immersed and indicate the pH range you wouldexpect. While indicators such as phenolphthalein and litmus are not an exact tool, they can give a general idea of the nature of a substance.

We work to identify liquids that would meet all these different pH values. Then we predict how they would react around common indicators. Work on figuring out how each pH level would react with Blue Litmus, Phenolphthalein, and Red Litmus.

Salts are given off as a byproduct as a result of a reaction between these two classes of liquids. The strong bases are the Group I and Group II hydroxides and most others are considered weak.Provide the missing chemical formulas and terms in the chart below.

Acids and bases are chemical substances that react with each other and may affect pH levels. Acids are characteristically sour, corrosive, and neutralized by bases. The definitions of acids and bases depend on the Arrhenius, Brnsted-Lowry, and Lewis theories.

For instance, the weak base ammonia (NH3), a common component of fertilizers, would not fit into the Arrhenius definition because it does not release OH-. Despite this, it is a base because it reacts with hydrochloric acid (HCl) acids.

Brnsted-Lowry acids are proton donors, while Brnsted-Lowry bases are proton acceptors. In this theory, a proton is defined as a single hydrogen ion (H+), and amphoteric substances act as both acids and bases. The definition of Brnsted-Lowry may apply to the Arrhenius substances.

While the Brnsted-Lowry theory is more inclusive than the Arrhenius, it still has limitations. It cannot explain why compounds like boron trifluoride (BF3) or aluminum (III) chloride (AlCl3) can act as acids without protons. It also does not cover reactions between acid and base oxides.

Three different definitions of acids and bases are based on Arrhenius, Brnsted-Lowry, and Lewis's theories. Each theory becomes increasingly comprehensive than the other. The most comprehensive one, Lewis's theory, allows scientists to identify substances better and thereby predict reactions.

Before viewing an episode, download and print the note-taking guides, worksheets, and lab data sheets for that episode, keeping the printed sheets in order by page number. During the lesson, watch and listen for instructions to take notes, pause the video, complete an assignment, and record lab data. See your classroom teacher for specific instructions.

This semester begins with the introduction of the mole. This important concept will be used during the remainder of the year as the basis for many calculations involving chemical reactions, solutions, and gases. In the units on thermochemistry and chemical kinetics, you will learn how energy is absorbed and given off during chemical reactions and how energy, and factors affect the rates of reactions. The study of reaction rates will lead you into the study of chemical equilibrium. In this semester, you will also study electrochemistry, from batteries to electroplating. And you will learn about acids, bases and salts. Unit 15 is a brief study of the atomic nucleus, which your teacher may introduce at any time during the year.

This worksheet lists 20 formulas. Students must label each formula as an "acid," "base," or "salt." All acids on this handout begin with H-. All bases on this handout end with -OH-. All other compounds are salts.

The acid ion

The base ion

pH value of an acid

pH value of a base

Neutral pH value

Acid taste

Base taste

Color of phenolthalein in an acid

Color of phenolthalein in a base

Technique used to find the unknown concentration of an acid solution

Feels slippery

Reacts with metals to produce hydrogen gas

Formed from neutralization

Reaction when the number of H+ = OH-

An example of an acid

An example of a base

An example of a salt

Color of litmus in an acid

Color of litmus in a base

Reference table of acids

pH that is 100X more acidic than a pH of 8

pH that is 100X more basic than a pH of 8

A matching sheet, or a matching quiz, is a sheet with two columns. In the first column there will be a word, statement or question, and in the second column are the answers, jumbled around in a different order.

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