Reference Tables: K, L, M, J, & T PACKET #10: Acids, Bases, and Salts Reference Tables: K, L, M, J, & T www.regentsprep.org

Characteristics of Acids: Table K Acids in an aqueous solution (in water) conducts electricity (acids are electrolytes). Acids cause color changes in acid-base indicators: Blue Litmus (turns red in an acid) Phenolphthalein (colorless in an acid) pH is less than 7 Acids react with bases to form a salt and water. This is called a Neutralization Reaction: a reaction when there is the same number of H+ ions as OH- ions; produce a salt and a water. Ex: HCl + NaOH  NaCl + H2O HBr + KOH  H2O + KBr

Characteristics of Acids Contains a high concentration of Hydrogen ions (H+) or Hydronium Ion (H3O+) - H2O + H+ = H3O+ Taste Sour lemons/citric acid vinegar/acetic acid carbonated drinks/carbonic acid Conduct Electricity The greater the concentration the better they conduct electricity If the acid is a good conductor of electricity it is called a strong acid If the acid is a poor conductor of electricity it is called a weak acid Corrosive – used to clean metals

Reactions of Acids With Metals: Acids react with certain metals to produce hydrogen gas (H2) Look at Reference Table J Activity Series Activity Decreases as you go Down Table J Metals Above Hydrogen will react with Hydrogen Containing Acids to produce a salt and hydrogen gas (H2)

Reactions of Acids with Metals Acids react with certain metals to produce hydrogen gas (H2) Look at Reference Table J Activity Series Activity Decreases as you go Down Table J Metals Above hydrogen will react with hydrogen containing acids to produce a salt and hydrogen gas (H2)

Characteristics of Bases: Table L Bases in an aqueous solution (in water) conducts electricity (bases are electrolytes). Bases cause color changes in acid-base indicators: Red Litmus (turns blue in an base) Phenolphthalein (pink in an base) pH is greater than 7 Bases react with acids to form a salt and water. This is called a Neutralization Reaction: a reaction when there is the same number of H+ ions as OH_ ions; produce a salt and a water. Ex: HCl + NaOH  NaCl + H2O HBr + KOH  H2O + KBr

Characteristics of Bases Contains a high concentration of Hydroxide ion (OH-) Taste Bitter Feel Slippery or Soapy Conduct Electricity The greater the concentration the better they conduct electricity If the base is a good conductor of electricity it is called a strong base If the base is a poor conductor of electricity it is called a weak base Caustic – dissolves skin

Beware of Tricks . . . Later, we will learn about Organic compounds, which are compounds that contain carbon. Two are organic acids and alcohols. Organic Acids have a functional group –COOH, so when you see a compound with carbon and this functional group it is an acid!! Ex: CH3COOH Alcohols have a functional group –OH (hyroxyl), not OH- (hydroxide); alcohols are not bases!! Ex: CH3OH

Table K Table L

Strong Acids & Bases HCl HBr HI HNO3 H2SO4 HClO3 HClO4. NaOH KOH Ca(OH)2 LiOH RbOH CsOH Ba(OH)2 NH3 is a weak base!!

Characteristics of Salts An ionic compound that has positive ions other than hydrogen (H+) and negative ions other than hydroxide (OH-). Example: NaCl (Na+ and Cl-). Salts conduct electricity (salts are electrolytes). ACIDS, BASES & SALTS ARE ELECTROLYTES

ARRHENIUS THEORY OF ACIDS & BASES Svante Arrhenius (Sweden); 1859-1927 An Arrhenius Acid has H and releases H+ in an aqueous solution. Example: HCl, HBr, H2SO4 The H+ ion is the only positive ion in these solutions. The H+ ions are always attached to H2O forming H3O+ (hydronium ions).

ARRHENIUS THEORY OF ACIDS & BASES An Arrhenius base has OH (hydroxide) and releases OH- (hydroxide ion) in an aqueous solution. Example: NaOH, KOH, Ca(OH)2 The OH- ion is the only negative ion in these solutions. Example: Which substances can be classified as an Arrhenius acid? 1. NaCl 2. HCl 3. LiOH 4. KOH

Bronsted-Lowry Theory (Alternate Acid-Base Theory) Johannes Bronsted (Denmark); 1879-1947 Thomas Lowry (England); 1874-1936 Acids: H+ donor (proton donors) Bases: H+ acceptor (proton acceptors) Bases Accept Acids Donate

Bronsted-Lowry Theory (Alternate Acid-Base Theory) Example: HCl(g) + H2O(l)  H3O+(aq) + Cl- (aq) HCl is the acid; donating H+ to H2O H2O is the base; accepts H+ to form H3O+ Try this one . . . HNO3(g) + H2O(l)  H3O+(aq) + NO3-(aq)

Conjugate Acid Base Pairs Two substances that are related to each other by the donating and accepting of a single proton. A conjugate base is what remains after the acid donates a proton A conjugate acid is what is formed when a base accepts a proton.

Conjugate Acid Base Pairs 1. Identify the acids, bases, and conjugate pairs in the following reaction. Explain your reasoning. NH4+ + OH- → NH3 + H2O 2. Identify the acids, bases, and conjugate pairs in the following reaction. Explain your reasoning. H3PO4 + NO2- → HNO2 + H2PO4- 3. Identify the acids, bases, and conjugate pairs in the following reaction. Explain your reasoning. HI (aq) + H2O (l) → H3O+ (aq) + I- (aq)

Amphoteric Substances An amphoteric substance can sometimes act like an acid and sometimes act like a base. Examples are H2O & HSO4 H2O + H2O  H3O+ + OH- (one water is an acid and one is a base) Water #1 is an acid (an H+ donor); OH- remains Water #2 is a base (an H+ acceptor); H3O+ remains

pH Scale Logarithmic scale indicating the acidity of a substance. A pH less than 7 is acidic; the lower the number the more acidic. A pH more than 7 is basic; the higher the number the more basic. A pH of 7 is neutral. 0-2 = strong acid 3-5 = medium strong acid 6 = weak acid 7 = neutral 8 = weak base 9-11 = medium strong base 12-14 = strong base

pH Scale Movement from one whole number to the next represents a change by a power of 10. Acids: 1-7, [H3O+] > [OH-] Neutral: 7, [H3O+] = [OH-] Bases: 7-14, [H3O+] < [OH-] EXAMPLE: Which pH change represents a hundredfold increase in the concentration of H3O+? 1. pH 5 to pH 7 2. pH 13 to pH 14 3. pH 3 to pH 1 4. pH 4 to pH 3

Meaning of pH pH = -log[H+] Example: Determine the pH of a solution in which the [H+] = 1.0X10-5 M. Is this solution acidic or basic? pH = -log[1.0X10-5] = -(-5) = 5 The solution is acidic.

Meaning of pH Example 2: An unknown solutions is found to have a hydronium ion concentration of 1.00X10-11 M. Is the solution acidic or basic? Example 3: What is the hydronium ion concentration of a solution with a pH of 7?

pH Indicators – Table M Indicators change color when pH changes. They show whether a solution is an acis or base and how strong. Methyl orange: turns red in a solution with pH of 3.2 or less. It turns yellow in when pH is 4.4 or more. Between 3.1 and 4.4 is a blended color (orange). Bromthymol blue: turns yellow in a solution with pH of 6.0 or less (acidic) and turns blue in base with a pH of 7.6 or more. Bromcresol green: turns yellow in a solution with pH 3.8 or less. It turns blue in a solution with pH 5.4 or more. You can use more than one indicator to really pin point the pH

Neutralization Reactions In neutralization reactions an Arrhenius Acid and an Arrhenius Base react to form Salt and Water.

Neutralization Reactions NaOH + HCl  NaOH + HNO3  Ca(OH)2 + H2SO4  H3PO4 + Mg(OH)2  HC2H3O2 + Al(OH)3  H2CO3 + KOH 

Titration Titration is a lab process in which a volume of a solution of known concentration is used to determine the concentration of another solution. Titration is a practical application of a neutralization reaction. A titration reaction involves a complete neutralization reaction where the moles of H+ equals the moles of OH- An indicator previously added to the solution, such as litmus or phenolphthalein, indicates the change from acid to neutral or basic to neutral.

Titration Procedure Place a measured amount of acid or base of unknown concentration in a flask and add two drops of phenolphthalein Use a ring stand with a burette clamp and a burette as shown in the diagram to the right. Fill the burette with a standard solution (an acid or base of known concentration) The burette is used to measure the amount of standard solution that is dispensed

Titration Procedure Continued… (#H+) MAVA =MBVB (#OH-) Hold the flask containing the acid or base of unknown concentration under the burette. Run the standard solution slowly into the flask, mixing occasionally by swirling. When the color begins to change on contact with the standard solution, add the standard solution one drop at a time until one final drop causes a complete and permanent color change. Determine the volume of standard solution used Calculate the concentration of the unknown solution using the data you gathered and the equation (Table T) (#H+) MAVA =MBVB (#OH-)

(#H+) MAVA =MBVB (#OH-) Neutralization Means (H+ = OH-) MA = molarity of H+ VA = volume of acid MB = molarity of OH- VB =  volume of base

Example 1: What is the molarity of HCl (aq) if 10. milliliters of 4.0 M NaOH (aq) neutralizes exactly 20. milliliters of HCl (aq)?

Example 2: What is the molarity of NaOH (aq) if 10. milliliters of 2 M HBr (aq) neutralizes exactly 5. milliliters of NaOH (aq)?

Review Questions 1) When an Arrhenius acid dissolves in water, the only positive ion in the solution is A) H+ B) K+ C) Li+ D) Na+ 2) Which ion is the only negative ion present in an aqueous solution of an Arrhenius base? A) hydrogen ion B) hydride ion C) hydroxide ion D) hydronium ion

3) Which substance is an Arrhenius base? A) CH3OH B) CH3Cl C) KOH D) KCl 4) Given the reaction: NH3 + HCl  NH4Cl In this reaction, ammonia molecules (NH3) act as a base because they A) accept hydroxide ions (OH-) B) donate hydroxide ions (OH-) C) donate hydrogen ions (H+) D) accept hydrogen ions (H+) 5) Which of these pH numbers indicates the highest level of acidity? A) 12 B) 10 C) 5 D) 8

6) Which of these 1 M solutions will have the highest pH? A) NaCl B) CH3OH C) HCl D) NaOH 7) Which equation represents a neutralization reaction? A) H2SO4 + Mg(OH)2  MgSO4 + 2H2O B) Na2CO3 + CaCl2  2NaCl + CaCO3 C) Ni(NO3)2 + H2S  NiS + 2HNO3 D) NaCl + AgNO3  AgCl + NaNO3 8) A student neutralized 16.4 milliliters of HCl by adding 12.7 milliliters of 0.620 M KOH. What was the molarity of the HCl acid? A) 0.801 M B) 0.620 M C) 0.480 M D) 0.168 M

9) How many milliliters of 0 9) How many milliliters of 0.100 M NaOH(aq) would be needed to completely neutralize 50.0 milliliters of 0.300 M HCl(aq)? A) 16.7mL B) 300.mL C) 50.0 mL D) 150. mL 10) Given the reaction at equilibrium: HSO-4 + H2O > H3O+ + SO4-2 The two Bronsted bases are A) H2O and H3O+ B) H3O+ and SO4-2 C) H2O and SO4-2 D) H3O+ and HSO-4

11) If a solution has a hydronium ion concentration of 1 x 10-9 M, the solution is A) basic and has a pH of 5 B) basic and has a pH of 9 C) acidic and has a pH of 9 D) acidic and has a pH of 5 12) Which relationship between ion concentrations always exists in an aqueous solution that is basic? A) [H+] is less than [OH-]. B) [H+] equals zero. C) [H+] equals [OH-]. D) [H+] is greater than [OH-].

13) A student recorded the following buret readings during a titration of a base with an acid: Calculate the molarity of the KOH. [Show all work. Record your answer to the correct number of significant figures.]