高雄醫學大學九十二學年度學士後醫學系招生考試試題 科目:化學 考試
... 66. Calculate the temperature at which the average kinetic energy of O2 gas is twice that of He gas at 10℃. (A) 2.50℃ (B) 10.0℃ (C) 20.0℃ (D) 160℃ (E) 293℃ 67. The sodium salt, NaA, of a weak acid is dissolved in water; no other substance is added. Which of the statements (to a close approximation) ...
... 66. Calculate the temperature at which the average kinetic energy of O2 gas is twice that of He gas at 10℃. (A) 2.50℃ (B) 10.0℃ (C) 20.0℃ (D) 160℃ (E) 293℃ 67. The sodium salt, NaA, of a weak acid is dissolved in water; no other substance is added. Which of the statements (to a close approximation) ...
Energy and Matter in Chemical Change Science 10
... (Ag) and copper (Cu) are some of the most efficient metals and are often used in electronics. 2. Reactivity: Metals are very reactive, some more than others, but most form compounds with other elements quite easily. Sodium (Na) and potassium (K) are some of the most reactive metals. 3. Chemical: Met ...
... (Ag) and copper (Cu) are some of the most efficient metals and are often used in electronics. 2. Reactivity: Metals are very reactive, some more than others, but most form compounds with other elements quite easily. Sodium (Na) and potassium (K) are some of the most reactive metals. 3. Chemical: Met ...
2.0 Chem 20 Final Review
... ▫ Hydrogen nucleus (proton) is simultaneously attracted to two pairs of electrons; one closer (in the same molecule) and one further away (a lone pair on the next molecule) Why do you need a strongly electronegative atom? It pulls the hydrogen’s ...
... ▫ Hydrogen nucleus (proton) is simultaneously attracted to two pairs of electrons; one closer (in the same molecule) and one further away (a lone pair on the next molecule) Why do you need a strongly electronegative atom? It pulls the hydrogen’s ...
E:\My Documents\sch4u\SCH4U review McKay answers.wpd
... bent 1 single 1 double 1 lone pair non-polar (1 co-ord) ...
... bent 1 single 1 double 1 lone pair non-polar (1 co-ord) ...
Infant formula
... Compared with GB 10765-1997, GB 10766-1997 and GB 10767-1997, the following changes have been made to the Standard: ——Integrate the above three standards to one, titled as “Infants Formula”; ——Provisions therein are modified. Annex A and Annex B of this present National Standard is informative. The ...
... Compared with GB 10765-1997, GB 10766-1997 and GB 10767-1997, the following changes have been made to the Standard: ——Integrate the above three standards to one, titled as “Infants Formula”; ——Provisions therein are modified. Annex A and Annex B of this present National Standard is informative. The ...
1.02 x 10 = 3 mol lit 3.4 x 10
... CH3COOH CH3COO + Na+ Due to common ion effect of CH3COO- Hydrogen ion concentration [H+] decreases. So the pH value increases. (ii) Calculate the pH of an aqueous solution of ammonium formate assuming complete dissociation. (pKa for formic acid = 3.8 and pKb for ammonia = 4.8) Ans: Ammonium format ...
... CH3COOH CH3COO + Na+ Due to common ion effect of CH3COO- Hydrogen ion concentration [H+] decreases. So the pH value increases. (ii) Calculate the pH of an aqueous solution of ammonium formate assuming complete dissociation. (pKa for formic acid = 3.8 and pKb for ammonia = 4.8) Ans: Ammonium format ...
Chemical Equilibrium - Chemistry Teaching Resources
... The strong base will have dissociated completely meaning that all the OH—(aq) ions were available to react with the Fe3+(aq) ions . The weak base is only partially dissociated so less than 1% of the OH—(aq) ions are available at the beginning. However, as the OH—(aq) ions react with Fe3+(aq) they ...
... The strong base will have dissociated completely meaning that all the OH—(aq) ions were available to react with the Fe3+(aq) ions . The weak base is only partially dissociated so less than 1% of the OH—(aq) ions are available at the beginning. However, as the OH—(aq) ions react with Fe3+(aq) they ...
- Catalyst
... – a solid precipitate forms when aqueous solutions of certain ions are mixed • Acid-Base: proton transfer reactions – acid donates a proton to a base, forming a molecule (water or another weak acid) and an aqueous salt – Acid: proton-donor; Base: proton-acceptor • Oxidation-Reduction: electron trans ...
... – a solid precipitate forms when aqueous solutions of certain ions are mixed • Acid-Base: proton transfer reactions – acid donates a proton to a base, forming a molecule (water or another weak acid) and an aqueous salt – Acid: proton-donor; Base: proton-acceptor • Oxidation-Reduction: electron trans ...
Acid-Base Equilibria - Riverside Local Schools
... when the base accepts a proton. Two such species that differ from each other only by the presence or absence of a proton together are known as a conjugate acid-base pair. Autoionization of water produces small concentrations of hydronium and hydroxide ions in pure water. The equilibrium constant for ...
... when the base accepts a proton. Two such species that differ from each other only by the presence or absence of a proton together are known as a conjugate acid-base pair. Autoionization of water produces small concentrations of hydronium and hydroxide ions in pure water. The equilibrium constant for ...
Common Student Misconceptions
... • Compounds containing alkali metal ions or ammonium ion are soluble. • Compounds containing NO3– or C2H3O2– are soluble. • Compounds containing Cl–, Br– or I– are soluble. • Exceptions: Compounds of Ag+, Hg22+, and Pb2+. • Compounds containing SO42– are soluble. • Exceptions: Compounds of Sr2+, Ba2 ...
... • Compounds containing alkali metal ions or ammonium ion are soluble. • Compounds containing NO3– or C2H3O2– are soluble. • Compounds containing Cl–, Br– or I– are soluble. • Exceptions: Compounds of Ag+, Hg22+, and Pb2+. • Compounds containing SO42– are soluble. • Exceptions: Compounds of Sr2+, Ba2 ...
IChO 35 Theoretical Exam
... (b) HBr boils at a lower temperature than HI Y N (c) Pure HI can be produced by reacting concentrated sulfuric acid with KI. Y N (d) Ammonia solutions are buffer solutions because they contain the conjugate pair NH3 – NH4+. Y N (e) Pure water at 80°C is acidic. Y N (f) During electrolysis of an aque ...
... (b) HBr boils at a lower temperature than HI Y N (c) Pure HI can be produced by reacting concentrated sulfuric acid with KI. Y N (d) Ammonia solutions are buffer solutions because they contain the conjugate pair NH3 – NH4+. Y N (e) Pure water at 80°C is acidic. Y N (f) During electrolysis of an aque ...
CLASSES AND NOMENCLATURE OF INORGANIC COMPOUNDS
... C Heat Conductivity. D Opacity. E Conductivity ...
... C Heat Conductivity. D Opacity. E Conductivity ...
IGCSE Revision Guide (Double Award) | PDF
... Recall the charge on common ions – both metals and non-‐metals – and compound ions e.g. SO42-‐, CO32-‐ , NH4+ , NO3-‐ . Deduce the charge of an ion from the electronic configuration of the ...
... Recall the charge on common ions – both metals and non-‐metals – and compound ions e.g. SO42-‐, CO32-‐ , NH4+ , NO3-‐ . Deduce the charge of an ion from the electronic configuration of the ...
Net ionic equation
... 2 HClO4(aq) + Ca(OH)2(aq) Ca(ClO4)2(aq) + 2 H2O(l) HNO2(aq) + NaOH(aq) NaNO2(aq) + H2O(l) 2 HBr(aq) + Cu(OH)2(s) CuBr2(aq) + 2 H2O(l) The last reaction above illustrates why insoluble hydroxide compounds are considered insoluble bases. Note that ionic compounds other than hydroxides (OH-) or o ...
... 2 HClO4(aq) + Ca(OH)2(aq) Ca(ClO4)2(aq) + 2 H2O(l) HNO2(aq) + NaOH(aq) NaNO2(aq) + H2O(l) 2 HBr(aq) + Cu(OH)2(s) CuBr2(aq) + 2 H2O(l) The last reaction above illustrates why insoluble hydroxide compounds are considered insoluble bases. Note that ionic compounds other than hydroxides (OH-) or o ...
Year End Review
... The next two questions deal with the identification and characterization of three elements which we shall call X, Y, and Z. The elements have successive atomic numbers each increasing by one in the order given. Atoms of element Z form stable ions with the formula Z+. 10. Which of the following stat ...
... The next two questions deal with the identification and characterization of three elements which we shall call X, Y, and Z. The elements have successive atomic numbers each increasing by one in the order given. Atoms of element Z form stable ions with the formula Z+. 10. Which of the following stat ...
corrected Amino acids and Protein
... iv) Zwitter ion: When the dipole moment of glycine is measured in aqueous solution, this value is found to be very large. To account for this large value it has been suggested that glycine consists, in solution, as an inner salt, as it has both basic –NH2 group and acidic –COOH group, it exists as d ...
... iv) Zwitter ion: When the dipole moment of glycine is measured in aqueous solution, this value is found to be very large. To account for this large value it has been suggested that glycine consists, in solution, as an inner salt, as it has both basic –NH2 group and acidic –COOH group, it exists as d ...
Chapter 04
... To determine the molecular, ionic and net ionic equations: 1) Write and balance the molecular equation, predicting the products by assuming that the cations trade anions. 2) Write the ionic equation by separating strong electrolytes into their ...
... To determine the molecular, ionic and net ionic equations: 1) Write and balance the molecular equation, predicting the products by assuming that the cations trade anions. 2) Write the ionic equation by separating strong electrolytes into their ...
CHEM110P1_06_2015_Y_P1
... Answer the following questions directly on the question paper in the space provided. Students are requested to write neatly and clearly to ensure accurate marking. ...
... Answer the following questions directly on the question paper in the space provided. Students are requested to write neatly and clearly to ensure accurate marking. ...
Estimate the strength of given sodium carbonate solution
... weak bases).They change their colour within a certain pH range. Considering two important indicators , Phenolphthalein: It is weak organic acid, pH range is from 8.3 to 10.5, in acid it is colourless and in base it is pink in colour. Methyl orange:It is a weak organic base, pH range is from 3.2 to 4 ...
... weak bases).They change their colour within a certain pH range. Considering two important indicators , Phenolphthalein: It is weak organic acid, pH range is from 8.3 to 10.5, in acid it is colourless and in base it is pink in colour. Methyl orange:It is a weak organic base, pH range is from 3.2 to 4 ...
Questions - Scheikundeolympiade
... (b) HBr boils at a lower temperature than HI Y N (c) Pure HI can be produced by reacting concentrated sulfuric acid with KI. Y N (d) Ammonia solutions are buffer solutions because they contain the conjugate pair NH3 – NH4+. Y N (e) Pure water at 80°C is acidic. Y N (f) During electrolysis of an aque ...
... (b) HBr boils at a lower temperature than HI Y N (c) Pure HI can be produced by reacting concentrated sulfuric acid with KI. Y N (d) Ammonia solutions are buffer solutions because they contain the conjugate pair NH3 – NH4+. Y N (e) Pure water at 80°C is acidic. Y N (f) During electrolysis of an aque ...
Document
... This section contains five (5) questions. You must answer all questions. Write your answers in the spaces provided below. Where questions require an explanation and/or description, marks are awarded for the relevant chemical content and also for coherence and clarity of expression. Lists or dot poin ...
... This section contains five (5) questions. You must answer all questions. Write your answers in the spaces provided below. Where questions require an explanation and/or description, marks are awarded for the relevant chemical content and also for coherence and clarity of expression. Lists or dot poin ...
Chapter 19: Acids and Bases
... You now know that HCl and HF are acids because they can donate a hydrogen ion in an acid-base reaction. From their chemical formulas, you can see that each acid can donate only one hydrogen ion per molecule. An acid that can donate only one hydrogen ion is called a monoprotic acid. Other monoprotic ...
... You now know that HCl and HF are acids because they can donate a hydrogen ion in an acid-base reaction. From their chemical formulas, you can see that each acid can donate only one hydrogen ion per molecule. An acid that can donate only one hydrogen ion is called a monoprotic acid. Other monoprotic ...
1 [Turn Over Section A For each question there are four possible
... No other combination of statements is used as a correct response. 36. Use of the Data Booklet is relevant to this question. When iron filings are added to nitric acid, a yellow solution and nitrogen dioxide gas are formed. On the addition of ammonium thiocyanate to the resultant solution, a bloodred ...
... No other combination of statements is used as a correct response. 36. Use of the Data Booklet is relevant to this question. When iron filings are added to nitric acid, a yellow solution and nitrogen dioxide gas are formed. On the addition of ammonium thiocyanate to the resultant solution, a bloodred ...
Acid
An acid (from the Latin acidus/acēre meaning sour) is a chemical substance whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals (like calcium) to form salts. Aqueous solutions of acids have a pH of less than 7. Non-aqueous acids are usually formed when an anion (negative ion) reacts with one or more positively charged hydrogen cations. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.There are three common definitions for acids: the Arrhenius definition, the Brønsted-Lowry definition, and the Lewis definition. The Arrhenius definition defines acids as substances which increase the concentration of hydrogen ions (H+), or more accurately, hydronium ions (H3O+), when dissolved in water. The Brønsted-Lowry definition is an expansion: an acid is a substance which can act as a proton donor. By this definition, any compound which can easily be deprotonated can be considered an acid. Examples include alcohols and amines which contain O-H or N-H fragments. A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. Examples of Lewis acids include all metal cations, and electron-deficient molecules such as boron trifluoride and aluminium trichloride.Common examples of acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute solution of this liquid), sulfuric acid (used in car batteries), and tartaric acid (a solid used in baking). As these examples show, acids can be solutions or pure substances, and can be derived from solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.