NCEA Level 3 Chemistry (91392) 2015
... The pH of a solution is calculated from its [H3O+]. NaOH is an ionic solid that is a strong base and dissociates completely to produce a high OH– concentration (low [H3O+]). Since [OH–] is high / [H3O+] is low, the pH is high. NaOH → Na+ + OH– CH3NH2 is a weak base that partially reacts / dissociate ...
... The pH of a solution is calculated from its [H3O+]. NaOH is an ionic solid that is a strong base and dissociates completely to produce a high OH– concentration (low [H3O+]). Since [OH–] is high / [H3O+] is low, the pH is high. NaOH → Na+ + OH– CH3NH2 is a weak base that partially reacts / dissociate ...
File
... Metal-like but does not contain all metal characteristics A positively charged particle A negatively charged particle Substance which produces hydrogen ions in aqueous solution, proton donor Not printed, Answer not present ...
... Metal-like but does not contain all metal characteristics A positively charged particle A negatively charged particle Substance which produces hydrogen ions in aqueous solution, proton donor Not printed, Answer not present ...
pH - OCCC.edu
... To calculate the pH of a weak acid solution: Write the ionization equilibrium for the acid. Write the equilibrium constant expression and its numerical value. Set up a table showing initial concentration, change, equilibrium concentration. Substitute equilibrium concentrations into the equ ...
... To calculate the pH of a weak acid solution: Write the ionization equilibrium for the acid. Write the equilibrium constant expression and its numerical value. Set up a table showing initial concentration, change, equilibrium concentration. Substitute equilibrium concentrations into the equ ...
Chap. 4 - Chemical Reactions
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
AP Chemistry Note Outline
... 2. Balance atoms other than H & O 3. Balance oxygen by adding H2O to the side that needs O 4. Balance hydrogen by adding H+ to the side that needs H 5. Balance the charge by adding electrons 6. Make the number of electrons gained equal to the number lost and then add the two halfreactions 7. Cancel ...
... 2. Balance atoms other than H & O 3. Balance oxygen by adding H2O to the side that needs O 4. Balance hydrogen by adding H+ to the side that needs H 5. Balance the charge by adding electrons 6. Make the number of electrons gained equal to the number lost and then add the two halfreactions 7. Cancel ...
2007 - Thompson Rivers University
... burned in excess air, and it produces 4.190 g of carbon dioxide and 3.428 g of water. What is the empirical formula? (Molar Masses: CO2 = 44.01 g/mol; H2O = 18.02 g/mol) (a) (b) (c) → (d) ...
... burned in excess air, and it produces 4.190 g of carbon dioxide and 3.428 g of water. What is the empirical formula? (Molar Masses: CO2 = 44.01 g/mol; H2O = 18.02 g/mol) (a) (b) (c) → (d) ...
Chemical Equation Interpretations – Match the chemical equation
... D. When octane and oxygen gas are burned in our cards, carbon dioxide and water come out in the exhaust. E. Methanol , if ingested, reacts with oxygen to form formaldehyde, which is toxic. Water is also formed in this reaction. F. Liquid mercury evaporates to produce mercury vapor. G. Saturated fatt ...
... D. When octane and oxygen gas are burned in our cards, carbon dioxide and water come out in the exhaust. E. Methanol , if ingested, reacts with oxygen to form formaldehyde, which is toxic. Water is also formed in this reaction. F. Liquid mercury evaporates to produce mercury vapor. G. Saturated fatt ...
Chem 30A Final Exam
... 16. You are titrating an unknown quantity of sulfuric acid (H2SO4) with a 0.1950 M NaOH standard solution and you find it takes 32.50 mL to reach an endpoint (phenolpthalein color change). What is the amount of sulfuric acid present in moles? Hint: Write a balanced chemical reaction equation for th ...
... 16. You are titrating an unknown quantity of sulfuric acid (H2SO4) with a 0.1950 M NaOH standard solution and you find it takes 32.50 mL to reach an endpoint (phenolpthalein color change). What is the amount of sulfuric acid present in moles? Hint: Write a balanced chemical reaction equation for th ...
Saturday Study Session 1 1st Class Reactions
... ii. For the titration at the equivalence point, calculate the number of moles of each of the following that reacted: a. MnO4b. C2O42iii. Calculate the total number of moles of C2O42- that were present in the 100.0 mL of prepared solution. ...
... ii. For the titration at the equivalence point, calculate the number of moles of each of the following that reacted: a. MnO4b. C2O42iii. Calculate the total number of moles of C2O42- that were present in the 100.0 mL of prepared solution. ...
Chapter 4 Aqueous Reactions and Solution Stoichiometry
... 7. Which hydroxides are strong bases? Sr(OH)2, KOH, NaOH, Ba(OH)2 (a). KOH, Ba(OH)2 (b). KOH, NaOH (c). KOH, NaOH, Ba(OH)2 (d) Sr(OH)2, KOH, NaOH and Ba(OH)2 8. A neutralization reaction between an acid and a metal hydroxide produces __________. (a). water and a salt (b). hydrogen gas (c). precipita ...
... 7. Which hydroxides are strong bases? Sr(OH)2, KOH, NaOH, Ba(OH)2 (a). KOH, Ba(OH)2 (b). KOH, NaOH (c). KOH, NaOH, Ba(OH)2 (d) Sr(OH)2, KOH, NaOH and Ba(OH)2 8. A neutralization reaction between an acid and a metal hydroxide produces __________. (a). water and a salt (b). hydrogen gas (c). precipita ...
Midterm 1 Spring 2004
... F __One mole of carbon-12 weighs exactly 12 grams. __A solution containing a strong electrolyte conducts electricity. __A liter is a volume equal to 100 cm3. __The discovery of the nucleus assisted Dalton in his development of atomic theory. __A free proton has a mass of exactly one atomic mass unit ...
... F __One mole of carbon-12 weighs exactly 12 grams. __A solution containing a strong electrolyte conducts electricity. __A liter is a volume equal to 100 cm3. __The discovery of the nucleus assisted Dalton in his development of atomic theory. __A free proton has a mass of exactly one atomic mass unit ...
Physical chemistry advanced laboratory course
... The Eq.(2) can also be reformulated in differential form and the mole fraction can be replaced with molality mS (where S refers to saturated solution): d ln mS = ...
... The Eq.(2) can also be reformulated in differential form and the mole fraction can be replaced with molality mS (where S refers to saturated solution): d ln mS = ...
Session #31: homework Solution
... The structure of cysteine at pH = 7 shows that the side group is protonated. So we must conclude that even though the pKa is 8.33, the sulfhydryl (−SH) is acting as an acid. The isoelectric point, pI, is the pH at which the zwitterion is the dominant species. Let’s start with extreme acid conditions ...
... The structure of cysteine at pH = 7 shows that the side group is protonated. So we must conclude that even though the pKa is 8.33, the sulfhydryl (−SH) is acting as an acid. The isoelectric point, pI, is the pH at which the zwitterion is the dominant species. Let’s start with extreme acid conditions ...
CHM2045 Final Exam Review, Spring 2017
... Step 1: H2O + NaCl + NH3 + CO2 NH4Cl + NaHCO3 Step 2: 2 NaHCO3 Na2CO3 + CO2 +H2O. What is the percent yield of sodium carbonate in the above process if 50.0 g of NaCl were used in Step 1 and 100.0 g of sodium carbonate were collected in Step 2? ...
... Step 1: H2O + NaCl + NH3 + CO2 NH4Cl + NaHCO3 Step 2: 2 NaHCO3 Na2CO3 + CO2 +H2O. What is the percent yield of sodium carbonate in the above process if 50.0 g of NaCl were used in Step 1 and 100.0 g of sodium carbonate were collected in Step 2? ...
Tutorial 7
... Faraday's Law The number of grams reduced at the cathode or oxidized at the anode is given by: ...
... Faraday's Law The number of grams reduced at the cathode or oxidized at the anode is given by: ...
The Hydrogen Atom 22.1 Radial Wavefunction
... As with the infinite square well, it makes sense to let κ = −2~m E (negative inside the square root, now – bound states will have E < 0 and we want to make κ real). We want to define a new “coordinate” ρ ≡ κ r. The advantage is to render the coordinate variable itself unitless. Whenever we want to c ...
... As with the infinite square well, it makes sense to let κ = −2~m E (negative inside the square root, now – bound states will have E < 0 and we want to make κ real). We want to define a new “coordinate” ρ ≡ κ r. The advantage is to render the coordinate variable itself unitless. Whenever we want to c ...
Chapter 4
... Predict the products of some simple types of chemical reactions: combination, decomposition, displacement, and metathesis reactions. ...
... Predict the products of some simple types of chemical reactions: combination, decomposition, displacement, and metathesis reactions. ...
Unit 3 Revision Notes 213.00KB 2017-03-01 18
... When a strong alkali such as NaOH or KOH is dissolved in water, it produces dissolved OH- ions. e.g. NaOH = Na+(aq) + OH-(aq) A weak alkali is only partly ionised, e.g. ammonia NH3 + H2O = NH4+(aq) + OH-(aq) (the ionisation reaction is reversible) When an acid reacts with an alkali, the ionic equati ...
... When a strong alkali such as NaOH or KOH is dissolved in water, it produces dissolved OH- ions. e.g. NaOH = Na+(aq) + OH-(aq) A weak alkali is only partly ionised, e.g. ammonia NH3 + H2O = NH4+(aq) + OH-(aq) (the ionisation reaction is reversible) When an acid reacts with an alkali, the ionic equati ...
2009-10 Chemistry 1st Semester Final Exam Topics and Review
... 35. Write and balance the chemical equations for the following reactions. Include the physical states (aq, s, l, g) of the reactants and products. a. When zinc metal and sulfur powder are heated, they form solid zinc sulfide. b. When sodium metal is placed in a beaker of water, hydrogen gas and sodi ...
... 35. Write and balance the chemical equations for the following reactions. Include the physical states (aq, s, l, g) of the reactants and products. a. When zinc metal and sulfur powder are heated, they form solid zinc sulfide. b. When sodium metal is placed in a beaker of water, hydrogen gas and sodi ...
PH
In chemistry, pH (/piːˈeɪtʃ/) is a numeric scale used to specify the acidity or alkalinity of an aqueous solution. It is the negative of the logarithm to base 10 of the activity of the hydrogen ion. Solutions with a pH less than 7 are acidic and solutions with a pH greater than 7 are alkaline or basic. Pure water is neutral, being neither an acid nor a base. Contrary to popular belief, the pH value can be less than 0 or greater than 14 for very strong acids and bases respectively.pH measurements are important in medicine, biology, chemistry, agriculture, forestry, food science, environmental science, oceanography, civil engineering, chemical engineering, nutrition, water treatment & water purification, and many other applications. The pH scale is traceable to a set of standard solutions whose pH is established by international agreement.Primary pH standard values are determined using a concentration cell with transference, by measuring the potential difference between a hydrogen electrode and a standard electrode such as the silver chloride electrode.The pH of aqueous solutions can be measured with a glass electrode and a pH meter, or indicator.pH is the negative of the logarithm to base 10 of the activity of the (solvated) hydronium ion, more often (albeit somewhat inaccurately) expressed as the measure of the hydronium ion concentration.The rest of this article uses the technically correct word ""base"" and its inflections in place of ""alkaline"", which specifically refers to a base dissolved in water, and its inflections.