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acids bases salts
| Question | Answer |
|---|---|
| What are electrolytes? | Substances that form ions in water and conduct electricity |
| Why do aqueous electrolyte solutions conduct electricity? | |
| What is a salt? | An ionic compound made of positive and negative ions an ionic compound formed by neutralizing an acid with a base |
| What is the pH of an acid? | Less than 7 |
| What is the pH of a base? | Greater than 7 |
| What is the pH of a neutral solution? | 7 |
| In an acid, how do [H+] and [OH-] compare? | [H+] > [OH-] |
| In a base, how do [H+] and [OH-] compare? | [OH-] > [H+] |
| What gives acids their characteristic properties? | H+ ions |
| What gives bases their characteristic properties? | OH- ions |
| What do acids taste like? | Sour |
| What do bases taste like? | Bitter |
| How do bases feel? | Slippery |
| Are acids electrolytes? | Yes |
| Are bases electrolytes? | Yes |
| How do acids react with certain metals? | They produce hydrogen gas |
| What is the general formula for pH? | pH = -log[H+] |
| If [H+] = 1 × 10^-4 M, what is the pH? | 4 |
| If [H+] = 1 × 10^-8 M, what is the pH? | 8 |
| What does a pH below 7 indicate? | Acidic solution |
| What does a pH above 7 indicate? | Basic solution |
| What does a pH of 7 indicate? | Neutral solution |
| What are the products of a neutralization reaction? | Salt and water |
| What reacts in a neutralization reaction? | An acid and a base |
| What is the general neutralization equation? | Acid + Base → Salt + Water (NaCl + H2O) |
| How are binary acids named? | hydro + root + ic acid |
| How is HCl named? | Hydrochloric acid |
| How is HI named? | Hydroiodic acid |
| How is H2S named? | Hydrosulfuric acid |
| How are oxoacids named when the ion ends in -ate? | Change -ate to -ic acid |
| How are oxoacids named when the ion ends in -ite? | Change -ite to -ous acid |
| What is H2SO4 called? | Sulfuric acid |
| What is H2SO3 called? | Sulfurous acid |
| What is HClO called? | Hypochlorous acid |
| What is the Arrhenius definition of an acid? | Produces H+ ions in water |
| What is the Arrhenius definition of a base? | Produces OH- ions in water |
| What is the Bronsted-Lowry definition of an acid? | A proton donor |
| What is the Bronsted-Lowry definition of a base? | A proton acceptor |
| What must a Bronsted-Lowry base have? | A lone pair of electrons |
| What are the six strong acids? | HCl, HBr, HI, HClO4, H2SO4, HNO3 |
| What are strong bases? | Group 1 or Group 2 hydroxides |
| Is NaOH a strong base? | Yes |
| Is Mg(OH)2 a strong base? | Yes |
| What is a monoprotic acid? | An acid that can donate one H+ |
| What is a polyprotic acid? | An acid that can donate more than one H+ |
| What is a diprotic acid? | An acid that can donate two H+ |
| What is a triprotic acid? | An acid that can donate three H+ |
| Give an example of a monoprotic acid. | HCl |
| Give an example of a diprotic acid. | H2SO4 |
| Give an example of a triprotic acid. | H3PO4 |
| What is an amphoteric substance? | A substance that can act as either an acid or a base |
| What is the most common amphoteric substance? | Water |
| What is a conjugate acid-base pair? | Two species differing by one H+ |
| How do you find a conjugate base? | Remove one H+ from the acid |
| How do you find a conjugate acid? | Add one H+ to the base |
| What is the conjugate base of HCl? | Cl- |
| What is the conjugate base of HNO3? | NO3- |
| What is the conjugate acid of HSO4-? | H2SO4 |
| What is the conjugate acid of SO4^2-? | HSO4- |
| What happens to [H+] when pH decreases by 1 unit? | It increases by a factor of 10 |
| If pH decreases from 6 to 4, how many times does [H+] increase? | 100 times |
| What is the ion-product constant for water (Kw)? | 1 × 10^-14 |
| In pure water, what is [H+]? | 1 × 10^-7 M |
| In pure water, what is [OH-]? | 1 × 10^-7 M |
| What is the relationship between [H+] and [OH-]? | [H+][OH-] = 1 × 10^-14 |
| What is the relationship between pH and pOH? | pH + pOH = 14 |
| What is the formula for pOH? | pOH = -log[OH-] |
| If [OH-] = 1 × 10^-4 M, what is the pOH? | 4 |
| If [OH-] = 1 × 10^-4 M, what is the pH? | 10 |
| What is a titration? | A procedure used to determine concentration through neutralization |
| What condition exists at the endpoint of a neutralization titration? | Moles of H+ equal moles of OH- |
| What titration equation is used on the Regents? | MaVaia = MbVbib |
| What does ia represent in the titration equation? | Number of H+ ions produced by the acid |
| What does ib represent in the titration equation? | Number of OH- ions produced by the base |
| What are acid-base indicators used for? | Determining pH and titration endpoints |
| What color is litmus in an acidic solution? | Red |
| What color is litmus in a basic solution? | Blue |
| Which indicator is commonly used in titrations? | Phenolphthalein |
| What color is phenolphthalein in acidic solutions? | Colorless |
| What color is phenolphthalein in basic solutions? | Pink |
| What indicates the endpoint when using phenolphthalein? | A faint pink color that persists |
| What Regents equation should be memorized for acid-base titrations? | MaVaia = MbVbib |
| What Regents equation should be memorized for pH calculations? | pH = -log[H+] |
| What Regents equation should be memorized for pOH calculations? | pOH = -log[OH-] |
| What Regents relationship should be memorized between pH and pOH? | pH + pOH = 14 |
| What Regents relationship should be memorized between H+ and OH- concentrations? | [H+][OH-] = 1 × 10^-14 |
Created by:
markoii