Chapter 9: Acid-Base Balance

Acid is a kind of chemical which, when dissolved in water, decomposes into—

The hydrogen ion is also called—

Which of the following is the symbol of a hydrogen ion?

Which of the following is a concentrated acid?

Acid turns blue litmus into—

Which of the following statements about acid is correct?

Tamarind is sour because it contains—

The product of the reaction between a metallic oxide and an acid is—

$\mathrm{CaO + 2HCl \rightarrow X + H_2O}$. Here X is—

Acid undergoing reaction with a more reactive metal produces salt and—

Which of the following is a strong acid?

Which of the following is a weak acid?

The decomposition of strong acids in water is shown using—

The decomposition of weak acids in water is shown using—

At $25^\circ\mathrm{C}$, out of $1000$ molecules of $\mathrm{CH_3COOH}$, the number that decompose in water is—

Strong acids ionize in water—

Weak acids in aqueous solution have—

When the amount of acid in an acid-water mixture is greater than water, it is called—

When the amount of water in an acid-water mixture is greater than acid, it is called—

Carbolic acid (carbonic acid) and acetic acid are examples of—

Which acid is found in milk?

Soft drinks contain—

Citric acid is found in—

Vinegar contains—

Tea contains—

The acid generated by the stomach wall to decompose food is—

Excess secretion of $\mathrm{HCl}$ in an empty stomach causes—

The acids in foods help us by—

Pickles contain various acids that act as—

The food acids are weak acids; therefore they—

Touching the tongue with a laboratory acid will—

The corrosive property of acid means—

To test the acidic nature of tamarind or pickles using litmus, the colour change observed is—

Which of the following is NOT a property of dilute acid?

Three reactive metals that react with dilute acid to give hydrogen are—

$\mathrm{Mg + H_2SO_4 \rightarrow X + H_2}$. Here X is—

Identify the gas evolved when a reactive metal is dropped in dilute acid—

The reaction of dilute acid with metallic carbonate produces salt, water and—

$\mathrm{CaCO_3 + 2HCl \rightarrow CaCl_2 + H_2O + ?}$. The missing product is—

When carbon dioxide produced from a carbonate-acid reaction is passed into lime water, the lime water—

The lime water turns turbid because—

When excess $\mathrm{CO_2}$ is bubbled into the turbid lime water, it again becomes—

The compound responsible for the opaque appearance after excess $\mathrm{CO_2}$ is—

The reaction $\mathrm{CaCO_3 + CO_2 + H_2O \rightarrow}$—

Dilute sulfuric acid reacting with metallic carbonate produces—

Limestone reacting with dilute nitric acid produces—

The general products of the reaction between a metallic bicarbonate and a dilute acid are—

$\mathrm{Ca(HCO_3)_2 + 2HCl \rightarrow CaCl_2 + 2H_2O + ?}$. The missing product is—

$\mathrm{2NaHCO_3 + H_2SO_4 \rightarrow ? + 2H_2O + 2CO_2}$. The salt produced is—

$\mathrm{NaHCO_3 + HNO_3 \rightarrow}$—

Sodium bicarbonate is also known as—

Calcium bicarbonate $[\mathrm{Ca(HCO_3)_2}]$ in water is—

The reaction $\mathrm{NaOH + HCl \rightarrow NaCl + H_2O}$ is called—

The metal oxides that react with acids are usually—

$\mathrm{H_2SO_4 + CuO \rightarrow ? + H_2O}$. The salt produced is—

The reaction of $\mathrm{CaO}$ with dilute $\mathrm{HNO_3}$ produces—

The salt produced when copper oxide reacts with dilute sulfuric acid is—

$\mathrm{CaO}$ is classified as—

A dry blue litmus paper placed on dehydrated oxalic acid lattice will—

Dry oxalic acid does not change litmus because it does not contain free—

Citric acid in aqueous solution—

Pure $\mathrm{H_2SO_4}$ and pure $\mathrm{HNO_3}$ in molecular state—

The colour of pure sulfuric acid and pure nitric acid in liquid state is—

The acidic property of a solution depends on the presence of—

Compared to a weak acid, a strong acid produces—

Hydrogen chloride dissolved in water becomes—

The fully ionized form of hydrochloric acid in water is represented by—

The acid that contains comparatively less water is called—

Which of the following is the protective gear required while using concentrated acids?

The bottle of concentrated nitric acid is brown because—

The gas dissolved in water to prepare concentrated hydrochloric acid is—

According to the chapter, concentrated nitric acid is prepared by dissolving in water—

According to the chapter, concentrated sulfuric acid is prepared by dissolving in water—

Opening the cork of a concentrated $\mathrm{HCl}$ bottle produces—

Which of the following acids is colourless in pure liquid state but is stored in a brown bottle?

Which of the following best defines a base?

Which of the following is NOT a base?

The reaction of $\mathrm{2KOH}$ with $\mathrm{H_2SO_4}$ produces—

Which of the following is a base?

Ammonium hydroxide $\mathrm{(NH_4OH)}$ is considered a base because—

Which of the following ions behave like reactive metal ions in producing ionic compounds?

Reaction between an acid and a base is called—

Glass cleaners in our homes commonly contain the base—

Toilet cleaners often contain the base—

Ferrous oxide is represented by the formula—

According to the chapter, the two conditions for a compound to be an alkali are—

Which of the following is an alkali?

Why is $\mathrm{Fe(OH)_2}$ NOT an alkali?

Why is $\mathrm{CaO}$ NOT an alkali?

Which of the following statements is correct?

Which of the following pairs are both alkalis?

The compound $\mathrm{NH_4OH}$ is an alkali because—

The action of a basic solution on red litmus is—

The action of a basic solution on blue litmus is—

Dilute base feels—

Dilute base solution is prepared by adding—

Direct contact of base with skin can—

The reaction $\mathrm{Al(NO_3)_3 + 3NaOH \rightarrow Al(OH)_3 \downarrow + 3NaNO_3}$ produces a precipitate that is—

The reaction of dilute $\mathrm{NaOH}$ with $\mathrm{Fe(NO_3)_2}$ gives a precipitate that is—

The reaction of dilute $\mathrm{NaOH}$ with $\mathrm{Fe(NO_3)_3}$ gives a precipitate that is—

The reaction of dilute $\mathrm{NaOH}$ with $\mathrm{Cu(NO_3)_2}$ gives a precipitate that is—

The reaction of dilute $\mathrm{NaOH}$ with $\mathrm{Zn(NO_3)_2}$ gives a precipitate that is—

In the reaction $\mathrm{Cu(NO_3)_2 + 2NaOH \rightarrow Cu(OH)_2 + 2NaNO_3}$, sodium nitrate—

The general type of products formed when alkali (NaOH) reacts with metallic nitrates is—

In the reaction with $\mathrm{Al(NO_3)_3}$, the molar ratio of $\mathrm{NaOH}$ required is—

$\mathrm{NH_4Cl + NaOH \rightarrow ?}$—

The characteristic gas produced when alkali reacts with an ammonium salt is—

$\mathrm{2NH_4Cl + Ca(OH)_2 \rightarrow ?}$—

$\mathrm{NH_4Cl + KOH \rightarrow}$—

The characteristic detection test for an ammonium salt uses—

In the solid state, ions of $\mathrm{KOH}$ and $\mathrm{NaOH}$ are—

Once dissolved, $\mathrm{NaOH}$ in water gives—

The negative charge in alkali solution is carried by—

Ammonia gas dissolved in water gives—

The alkalis that dissolve partially in water are called—

Strong alkali in aqueous solution is—

Concentrated acids and concentrated alkali are highly—

To prepare dilute solution from concentrated acid one must—

If concentrated acid splashes on skin, the first response should be to—

Concentrated acid and alkali can damage the—

In the conductivity experiment, two graphite rods are connected to a battery and a—

The bulb in the beaker containing dilute $\mathrm{HCl}$ glows brighter than the bulb in the beaker containing dilute $\mathrm{CH_3COOH}$ because—

A weak alkali in the conductivity experiment will give—

The conductivity experiment proves that $\mathrm{NaOH}$ is—

The amount of electricity conducted in an acidic solution depends primarily on—

pH stands for—

The mathematical expression for pH is—

In pH the letter "p" is written with a—

The molarity of $\mathrm{H^+}$ in 1 litre of distilled water is—

The pH of pure distilled water at room temperature is—

If the $\mathrm{[H^+]}$ in a solution rises to $10^{-6}$ mol/L, the pH becomes—

If $\mathrm{[H^+]}$ drops to $10^{-10}$ mol/L, the pH becomes—

As $\mathrm{[H^+]}$ increases, pH—

The pH of an acidic solution is—

The pH of an alkaline solution is—

The pH scale ranges from—

The strongest acid on the pH scale has the value—

The strongest alkali on the pH scale has the value—

The mixture of various acid and base indicators is called—

To measure the approximate pH of an unknown solution using a universal indicator we—

The instrument that gives a digital readout of pH is—

Litmus paper is used as—

According to the chapter, vegetables/flowers used to prepare home-made pH paper include—

To prepare home-made pH paper, the filter paper is dipped in the coloured extract and then—

The best pH range of soil for plant growth is—