Acids and Bases Ch 20,21 – Flashcards
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Unlock answers| Which ion(s) have the wrong charge? Na+, Mg+ or Al+ ? |
| Mg+ should be Mg2+ and Al+ should be Al3+ Charges are at the top of the columns of the periodic table. |
| Ionic compounds are made of: |
| positive ions and negative ions. |
| Ions form when neutral atoms gain or lose: |
| electrons, in order to be like a noble gas. |
| Ionic compounds always start with a: |
| metal, except for the one polyatomic NH4+1 |
| Which ion(s) have the wrong charge? Li-, O 2- , S2+ ? |
| Li should be Li1+, and sulfur should be S2-. The charges are at the top of the periodic table. |
| Which of the following polyatomics is correct? NH+4, OH-1, PO3-2 ? |
| OH-1 you may use the polyatomic chart on the test. |
| What does the suffix ‘-ate’ or ‘ite’ indicate in the name of the compound? |
| that there is a polyatomic for the anion, and there are oxygens in the polyatomic. |
| hydrogen ions or also called hydronium ions |
| What acids release into the water in which they are dissolved. |
| If an acid’s anion ends with ‘–ide’ such as |
| The prefix ‘hydro’ is used in the acid name. |
| HCl(gas)= hydrogen chloride gas THEN: |
| HCl(gas) in water causes the water to be called hydrochloric acid. |
| If a polyatomic is the anion of the acid, then: |
| There’s NO prefix of ‘hydro’. |
| If an acid’s polyatomic ends with ‘-ate’ such as H2SO4 = hydrogen sulfate THEN: |
The acid’s name ends with ‘-ic’. hydrogen sulfate = H2SO4 = sulfuric acid |
| If an acid’s polyatomic ends with ‘ite’ such as H2SO3 = hydrogen sulfite THEN: |
The acid’s name ends with ‘-ous’. hydrogen sulfite = H2SO3 = sulfurous acid |
| Phosphoric acid is: Phosphorous acid is: |
hydrogen phosphate = H3PO4= Phosphoric acid hydrogen phosphite = H3PO3= Phosphorous acid |
| sour taste, electrolyte, litmus paper(pink), reacts with bases to make water and salt |
| properties of acids |
| slippery, bitter taste, electrolyte, litmus paper(blue), reacts with acids to make water and salt |
| properties of bases |
| 1+ is the charge of which acid ion? NH4 or H3O |
H3O1+ is called ‘hydronium ion’ & is acidic. NH41+ is called ‘ammonium ion’ and is a base. |
| If the hydrogen ion concentration is 1 x 10-9M then the solution is: |
| a base with a pH of 9. |
| If the hydrogen ion concentration is 1 x 10-4M, then the solution is: |
| an acid with a pH of 4. |
| If the hydrogen ion concentration is 1 x 10-4M, then what is the hydroxide ion concentration? |
| [OH-] = 1 x 10-10M and has a pH of 4. |
| If the hydroxide ion concentration is 1 x 10-6 M, then the hydrogen ion concentration is: |
| [H+] = 1 x 10-8 M and has a pH of 8. |
| The symbol for ‘concentration’ is: |
| brackets…[ ] |
| The concentration of hydronium ions in a neutral solution is: |
| [H+] = 1 x 10-7 M and has a pH of 7. |
The formula for pH is: example, hydronium concentration = [2.8 x 10-3M] |
pH = -log [H ion] and would be keyed into the calculator as: 2.8 EE 3 ± log ± = 2.6 and would be acidic |
What is the pH of a solution that has a hydronium concentration of 4.8 x 10-7M? |
| 4.8 EE 7 ± log ± = 6.3 and would be acidic |
What is the pH of a solution that has a hydronium concentration of 1.3 x 10-9M? |
| 1.3 EE 9 ± log ± = 8.8 and would be basic |
| What is the pH of [10-11M]? |
| 1 EE 11 ± log ± = 11 and would be basic |
| When the pH of a solution is between 0 and 6.99, the solution is: |
| acidic, pH < 7 |
| When the pH of a solution is between 7.1 and 14, the solution is: |
| basic, pH > 7 |
| When the pH of a solution is exactly 7 the solution is: |
| neutral |
When the hydronium ion concentration is 1x10-7M. |
| neutral or pH 7. |
| pH 3 is ten times _____ than pH 4 |
| more concentrated, both are acids |
| pH 6 is ten times _____ than pH 5 |
| more diluted, both are acids |
| pH 9 is ten times _____than pH 8 |
| more concentrated. both are bases |
| pH 8 is 100 times ______ than pH 10 |
| more diluted, both are bases |
| ‘diluted’ means |
| watered down |
| ‘strong’ acid means |
| ionizes completely in water….example: HCl and H2SO4 |
| ‘weak’ acid means |
| doesn’t ionize completely in water…some of the + and – ions won’t let go of each other….example: vinegar |
| ‘strong’ base means |
| ionizes completely in water….example: NaOH |
| ‘weak’ base means |
| doesn’t ionize completely in water…some of the + and – ions won’t let go of each other…..examples: NH4+ |
| acid + base = |
| salt + water |
| ionic compounds are always called: |
| salts |
| Acids start with a ________ that is acting like a metal. |
| hydrogen |
| Bases usually end with the polyatomic…. |
| hydroxide or (OH) |
| What is a titration? |
| a way to figure the concentration of an acid or a base. |
| neutralization |
| mixing an acid to a base to produce a salt and water. |
| buffer |
| a solution in which pH is kept relatively constant |
| diprotic acids |
| have two hydrogens in front or two ionizable protons, such as H2SO4 |
| pH |
| negative logarithm of the hydrogen ion concentration |
| acid theory…hydrogen-ion donor |
| Bronsted-Lowry acid (medium theory) |
| acid theory…can accept an electron pair |
| Lewis acid (hardest theory) |
| acid theory…dissociates into hydrogen ions |
| Arrhenius acid (simplest theory) |
| triprotic acid |
| have three hydrogens in front or three ionizable protons |
| monoprotic acid |
| has one hydrogen in front or one ionizable proton |
| Keeps the pH of a solution constant |
| buffer |
| H+ + OH- > H2O |
| summary of acid to base reaction |
| burette |
| measuring instrument for titrations |
| ‘pH indicator’ examples: |
| phenolphthalein, pH paper, red cabbage juice, bromthymol blue, and several others. |
| How to find the products of an acid to base being combined: Example: HZ + ROH> |
one product will be water…the result of the acid’s ‘H’ and the base’s ‘OH’. The other product is the cation of the base and the anion of the acid….RZ. |
Correctly written skeleton equation for the acid to base reaction: H2Z + R(OH)3 > |
H2Z + R(OH)3 > H2O + R2Z3….. Where Z could be sulfate and R could be aluminum. |
Correctly written skeleton equation for the acid to base reaction: H3Z + R(OH)2 > |
H3Z + R(OH)2 > H2O + R3Z2….. Where Z could be phosphate and R could be magnesium. |
Correctly written skeleton equation for the acid to base reaction: H1Z + R(OH)1 > |
H1Z + R(OH)1 > H2O + R1Z1….. Where Z could be chlorine and R could be sodium. |
| how to find the subscripts of a compound |
criss-cross the superscripts downward, but don’t take the + or – downward. |
| how to find the superscripts of a compound |
| look at the top of a periodic table and/or a polyatomic chart |
how to balance a skeleton equation such as: H3PO4 + Mg(OH)2 → H2O + Mg3(PO4)2 |
2H3PO4 + 3Mg(OH)2 → 6H2O + 1Mg3(PO4)2 |
| The coefficients of a balanced equation are also called: |
| moles of a balanced equation. |
| another way to write 1x10-8M. |
| 10-8M |
| hydronium ion symbols are: |
H3O+ or H3O+1 or H3O1+ [image] |
| What does the ‘M’ of 3M HCl mean? |
| The ‘M’ stands for ‘molar’ which tells how concentrated or diluted the HCl is. |
| another way to write 1x10-6M |
| 0.000001M |
which number is bigger? 0.0001 or 0.001 |
| 0.001 is bigger |
which number is bigger? 10-4 or 10-3 |
| 0.001 which is 10-3 is bigger than 0.0001 which is 10-4 |
