Chemistry Reaction of Acids and Bases

Calcium bicarbonate is formed, which is soluble in water.

Limestone, chalk, and marble.

Salt, carbon dioxide, and water.

<p>Phenolphthalein.</p> Signup and view all the answers

<p>The pink color disappears.</p> Signup and view all the answers

<p>The reaction between an acid and a base to form salt and water.</p> Signup and view all the answers

<p>Base + Acid → Salt + Water</p> Signup and view all the answers

<p>Copper oxide.</p> Signup and view all the answers

<p>Blue-green.</p> Signup and view all the answers

<p>Salt and water.</p> Signup and view all the answers

<p>$K_2CO_3(s) + 2HCl(aq) \rightarrow 2KCl(aq) + CO_2(g) + H_2O(l)$</p> Signup and view all the answers

<p>The properties of an acid and base are nullified. The acid donates $H^+$ ions and the base accepts $H^+$ ions to produce water.</p> Signup and view all the answers

<p>Magnesium sulfate ($MgSO_4$) and water ($H_2O$).</p> Signup and view all the answers

<p>Initially, the limewater turns milky due to the formation of calcium carbonate ($CaCO_3$). With continued bubbling, $CaCO_3$ dissolves to form $Ca(HCO_3)_2$, making the solution clear again.</p> Signup and view all the answers

<p>Metal hydrogencarbonate + Acid → Salt + Carbon dioxide + Water</p> Signup and view all the answers

<p>The black copper (II) oxide dissolves. The solution turns blue-green due to the formation of copper(II) chloride ($CuCl_2$).</p> Signup and view all the answers

<p>The pH decreases as the acidic HCl neutralizes the basic NaOH. The reaction produces salt and water which brings the pH closer to 7.</p> Signup and view all the answers

<p>$2KOH(aq) + H_2SO_4(aq) \rightarrow K_2SO_4(aq) + 2H_2O(l)$</p> Signup and view all the answers

<p>It is an indicator. It shows the acidity or basicity of the solution. It is pink in basic solutions and colorless in acidic solutions.</p> Signup and view all the answers

<p>Acid rain (containing acids like $H_2SO_4$) reacts with calcium carbonate ($CaCO_3$) in limestone, dissolving the stone. $CaCO_3(s) + H_2SO_4(aq) \rightarrow CaSO_4(aq) + H_2O(l) + CO_2(g)$</p> Signup and view all the answers

<p>The reaction produces a salt, carbon dioxide, and water. While the immediate products aren't neutral, the formation of water signifies the neutralization aspect, as acid's protons are being reacted with carbonate from the metallic carbonate.</p> Signup and view all the answers

<p>The reaction dissolves the insoluble calcium carbonate ($CaCO_3$) into soluble calcium bicarbonate ($Ca(HCO_3)_2$), which leads to the erosion of limestone. It also increases the concentration of calcium ions in the water, causing it to become temporarily hard.</p> Signup and view all the answers

<p>Phenolphthalein is used because it changes color within a specific pH range (8.3-10.0), indicating the endpoint of the neutralization. The color change happens due to protonation or deprotonation of the phenolphthalein molecule, leading to a shift in its electronic structure and light absorption properties.</p> Signup and view all the answers

<p>The products are magnesium chloride ($MgCl_2$), carbon dioxide ($CO_2$), and water ($H_2O$). The balanced equation is: $MgCO_3(s) + 2HCl(aq) \rightarrow MgCl_2(aq) + CO_2(g) + H_2O(l)$.</p> Signup and view all the answers

<p>Metal oxides act as bases because the oxide ion ($O^{2-}$) can accept protons ($H^+$) from acids, forming water. This is similar to how hydroxide ions ($OH^−$) in traditional bases react with acids, leading to salt and water formation.</p> Signup and view all the answers

<p>A more green than blue color suggests the presence of excess chloride ions ($Cl^−$) in the solution. High chloride concentrations can alter the complex formed with copper(II) ions, shifting the solution's color towards green.</p> Signup and view all the answers

<p>When a strong acid reacts with a weak base (or vice versa), the resulting salt can undergo hydrolysis, affecting the pH. For example, the salt formed from a strong acid and weak base will hydrolyze to produce excess $H^+$ ions, resulting in a pH less than 7.</p> Signup and view all the answers

<p>The common ion effect decreases the solubility of $CaCO_3$. If a solution already contains $Ca^{2+}$ ions, the addition of $CaCO_3$ will shift the equilibrium towards precipitation of $CaCO_3$ to maintain the solubility product constant ($K_{sp}$), thus reducing its solubility.</p> Signup and view all the answers

<p>Sulfuric acid reacts with limestone to form calcium sulfate ($CaSO_4$), carbon dioxide ($CO_2$), and water ($H_2O$). Calcium sulfate is more soluble than calcium carbonate, and its formation causes the gradual erosion and disintegration of the limestone structure.</p> Signup and view all the answers

<p>Heating the solutions and testing for carbon dioxide ($CO_2$) evolution can differentiate them. $NaHCO_3$ decomposes upon heating to produce $CO_2$, while $Na_2CO_3$ does not under similar conditions. Bubbling evolved gas through limewater will turn it milky if $CO_2$ is present, indicating the original solution was $NaHCO_3$.</p> Signup and view all the answers

<p>The predominant silver-containing species will likely be $Ag(CO_3)_n^{2n-1}$ complexes.The equilibria involve dissolution of $Ag_2CO_3$, reaction with $CO_2$ to form $Ag(CO_3)_n^{2n-1}$, and complex formation equilibria involving $Ag^+$, $CO_3^{2-}$ and $HCO_3^-$</p> Signup and view all the answers

<p>Initial protonation of $CaCO_3$ forms $CaHCO_3^+$. $SO_2$ dissolves in water to form $H_2SO_3$, which further dissociates to $HSO_3^-$ and $SO_3^{2-}$. These sulfite species react with $Ca^{2+}$ and $HCO_3^-$ to form soluble calcium sulfite complexes, accelerating the dissolution process.</p> Signup and view all the answers

<p>The protocol involves reacting $MgCO_3$ with $CO_2$ saturated water in a closed system, measuring the concentration of $Mg^{2+}$ and $HCO_3^-$ using ICP-OES and ion chromatography respectively, then calculating $K_{eq}$ using activity coefficients to correct for ionic strength effects, with error analysis considering instrument calibration and solution preparation.</p> Signup and view all the answers

<p>The pH range of phenolphthalein (8.3-10.0) may not align with the equivalence point of weak acid-strong base titrations, leading to overestimation of the endpoint. Factors include acid strength, concentration, indicator concentration and temperature. Using a different indicator with a pH range closer to the equivalence point or employing derivative analysis of the titration curve are potential mitigations.</p> Signup and view all the answers

<p>The alkalinity arises from the hydrolysis of $CO_3^{2-}$ to form $HCO_3^-$ and $OH^-$, and the subsequent hydrolysis of $HCO_3^-$ to form $H_2CO_3$ and $OH^-$. The equilibrium constants ($K_b$) for these reactions and the concentration of $Na_2CO_3$ dictate the pH, with temperature influencing the equilibrium constants.</p> Signup and view all the answers

<p>If the acid is a strong reducing agent, it may reduce $Cu^{2+}$ in $CuO$ to $Cu^+ $ or even $Cu$, leading to the formation of species like $CuCl$ or metallic copper alongside $CuCl_2$, water, and possibly chlorine gas depending on the specific conditions.</p> Signup and view all the answers

<p>$H_2SO_4$ protonates the metal oxides and hydroxides on the bronze surface. Copper forms $Cu^{2+}$ ions, tin forms $Sn^{4+}$ ions, and zinc forms $Zn^{2+}$ ions. These metal ions dissolve, leading to pitting and structural weakening. Sulphate ions can also form insoluble metal sulphates, contributing to the formation of a patina layer.</p> Signup and view all the answers

<p>Initially, conductivity decreases due to the replacement of highly mobile $OH^-$ ions by less mobile $Cl^-$ ions. At the equivalence point, conductivity reaches a minimum. Beyond the equivalence point, conductivity increases linearly due to the excess of highly mobile $H^+$ ions from the strong acid.</p> Signup and view all the answers

<p>The buffer system involves the equilibrium $CO_3^{2-} + H^+ \rightleftharpoons HCO_3^-$, governed by the Henderson-Hasselbalch equation: $pH = pK_a + log([CO_3^{2-}]/[HCO_3^-])$. Addition of acid shifts the equilibrium to the right, consuming $CO_3^{2-}$, while addition of base shifts it to the left, generating $CO_3^{2-}$, thus resisting pH changes.</p> Signup and view all the answers

<p>$BaCO_3$ will precipitate first because it has a lower $K_{sp}$ than $CaCO_3$. As $CO_2$ is added, carbonate concentration increases. $BaCO_3$ will precipitate when $[Ba^{2+}][CO_3^{2-}] &gt; K_{sp}(BaCO_3)$, and only after $Ba^{2+}$ is largely depleted will $CaCO_3$ begin to precipitate.</p> Signup and view all the answers

<p>A reaction between an acid and a base that results in the formation of a salt and water.</p> Signup and view all the answers

<p>A salt and water.</p> Signup and view all the answers

<p>It converts the insoluble calcium carbonate into soluble calcium bicarbonate ($Ca(HCO_3)_2$).</p> Signup and view all the answers

<p>Phenolphthalein is a pH indicator; it is pink in basic solutions and colorless in acidic solutions. Adding acid neutralizes the base, causing the pH to drop and the indicator to become colorless.</p> Signup and view all the answers

<p>$CuO(s) + 2HCl(aq) \rightarrow CuCl_2(aq) + H_2O(l)$. Copper(II) oxide dissolves, and the solution turns blue-green due to the formation of copper(II) chloride.</p> Signup and view all the answers

<p>Sodium sulfate ($Na_2SO_4$) is formed. $2NaOH(aq) + H_2SO_4(aq) \rightarrow Na_2SO_4(aq) + 2H_2O(l)$</p> Signup and view all the answers

<p>By evaporating the solution; a solid salt ($BaCl_2$) would remain if a neutralization reaction occurred. Also, by measuring the temperature change; neutralization reactions are exothermic and are accompanied by the release of heat.</p> Signup and view all the answers

<p>$KHCO_3(s) + HNO_3(aq) \rightarrow KNO_3(aq) + H_2O(l) + CO_2(g)$</p> Signup and view all the answers

<p>Magnesium carbonate ($MgCO_3$) will react fastest. Down the group 2, the solubility of carbonates decreases. Magnesium ions have the highest charge density making the magnesium carbonate unstable, and hence react faster with hydrochloric acid.</p> Signup and view all the answers

<p>CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)</p> Signup and view all the answers

<p>Neutralization reaction</p> Signup and view all the answers

<p>The pink color of phenolphthalein would reappear.</p> Signup and view all the answers

<p>A salt is an ionic compound formed when an acid reacts with a base, where the hydrogen ion of the acid is replaced by a metal ion or another positive ion.</p> Signup and view all the answers

<p>Initially, CaCO3 (calcium carbonate) is formed, which makes the solution milky. With excess CO2, CaCO3 reacts to form soluble Ca(HCO3)2 (calcium bicarbonate), causing the solution to clear.</p> Signup and view all the answers

<p>CuO(s) + 2HCl(aq) → CuCl2(aq) + H2O(l)</p> Signup and view all the answers

<p>Approximately $13.37 °C$</p> Signup and view all the answers

<p>Neutralization reactions are crucial in wastewater treatment to neutralize acidic or basic effluents before discharge and also in the production of fertilizers. One example is using ammonia to neutralize sulfuric acid to produce ammonium sulfate, a common fertilizer.</p> Signup and view all the answers

<p>0.060 M</p> Signup and view all the answers

<p>The products are $2NaCl(aq)$, $H_2O(l)$, and $CO_2(g)$. The underlying principle is a double displacement reaction where carbonate reacts with acid to form carbonic acid, which then decomposes into water and carbon dioxide.</p> Signup and view all the answers

CaCO3 reacts with water and CO2 to form Ca(HCO3)2, soluble in water.

Metal carbonate or hydrogencarbonate reacts with acid to produce salt, carbon dioxide, and water.

When an acid reacts with a base to produce salt and water.

A substance that changes color in the presence of an acid or base.

Copper oxide reacts with hydrochloric acid to form copper(II) chloride and water.

Metal carbonates react with acids to produce salt, CO2, and water.

Hydrogencarbonates react with acids to give salt, water, and CO2.

Salts are produced when you mix acids with bases or carbonates.

Acid addition to a basic solution causes an observable color change.

A generalized equation representing the reaction of a base and an acid to yield salt and water.

Limestone is mainly composed of calcium carbonate (CaCO3).

A metal oxide reacts with an acid to form a salt and water.

Dissolving copper oxide in hydrochloric acid creates a blue-green copper(II) chloride solution.

The products of a reaction between an acid and a base are salt and water.

Phenolphthalein changes color in response to acidity, usually turning pink in basic solutions.

Sodium hydroxide (NaOH) reacts with hydrochloric acid (HCl) to form sodium chloride (NaCl) and water.

When a base reacts with an acid, it undergoes neutralization to form salt and water.

Acids react with carbonates to produce a salt, water, and carbon dioxide.

A general equation for metal oxide and acid reactions is: Metal oxide + Acid → Salt + Water.

Hydrogencarbonates react with acids to yield salt, CO2, and water.

Limestone, chalk, and marble are different forms of CaCO3.

The reaction between an acid and a base that produces salt and water.

Phenolphthalein changes color when an acid is added to a base.

Copper oxide reacts with hydrochloric acid to yield copper(II) chloride and water.

A common reaction format is: Base + Acid → Salt + Water.

Metal oxides react with acids to form salts and water.

Mixing copper oxide with hydrochloric acid turns solution blue-green.

Hydrogencarbonates react with acids to produce salt, CO2, and water.

Phenolphthalein becomes colorless in acidic medium.

Neutralisation is represented as: Base + Acid → Salt + Water.

Adding acid to phenolphthalein changes the color, indicating acidity.

Metal oxides react with acids resulting in salt and water.

Copper oxide dissolving in HCl creates a blue-green copper(II) chloride solution.

Acids react with carbonates to yield salt, carbon dioxide, and water.

Indicators like phenolphthalein show color changes in acidic or basic solutions.

Mixing NaOH and HCl produces NaCl and water, demonstrating neutralization.

Hydrogencarbonates react with acids to produce salt, CO2, and water.

Metal oxides react with acids following the pattern: Metal oxide + Acid → Salt + Water.

Limestone, chalk, and marble are varieties of CaCO3.

Metal oxides react with acids to yield salt and water.

Adding acid to a basic solution neutralizes the base, often changing its color.

Copper oxide dissolves in hydrochloric acid, changing the solution color to blue-green.

Metal carbonates react with acids to form salts, CO2, and water.

Mixing NaOH with HCl creates NaCl and water, demonstrating neutralization.

Indicators like phenolphthalein signal acidity or basicity through color changes.

The reaction of an acid with a base results in salt and water.

Hydrogencarbonates react with acids, producing salt, CO2, and water.

CaCO3 reacts with water and CO2 to form Ca(HCO3)2, which is soluble.

Acid + Base → Salt + Water; represents all neutralization reactions.

Phenolphthalein changes from pink in basic to colorless in acidic solutions.

Copper oxide dissolves in hydrochloric acid to form blue-green copper(II) chloride.

Adding NaOH neutralizes acid, restoring the pink color of phenolphthalein.

Hydrochloric acid neutralizes copper oxide, resulting in colored solution.

Metal carbonates with acid produce salt, water, and carbon dioxide.

An acid can nullify the basic effect, as seen with NaOH and HCl.