If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is root beer with a pH of 5.3? If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is a saline solution with a pH of 7.0?
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If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is root beer with a pH of 5.3?
If 0-2 pH is considered strongly acidic, 2-7 is weakly acidic, 7.0 is neutral, 7-12 is weakly basic and 12-14 is strongly basic. Then what is a saline solution with a pH of 7.0?
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- CH3CH2CO2H , Ką = 1.3 x 105 CH3CH2CO2 , Kp = 7.7 x 10-10 F, Kp = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For the reaction between propanoic acid (CH3CH2CO2H) and a solution containing fluoride ions (F"): (a) The name of the conjugate base produced is (b) The name of the conjugate acid produced is (c) The reaction is favoured (write 'reactant' or 'product'), because the reactants are the (write 'weaker' or 'stronger') set of acid and base.Which of the following weak acid solutions has the highest percentage ionization? 0.01 M HCN ( Ka = 6.2 × 10-10) 0.01 М Н2СОз (Ка%34.5 х 10-/) 0.01 M HNO2 (Ka = 4.0 x 10-4) 0.01 М НСНО2 (Ка3D 1.8 х 10-4) 0.01 M HOC1 ( Ka = 3.5 × 10-8)Josephine reacts 10.0 mL of 0.50 M HCI with 10.0 mL of 0.50 M KOH. The solution experienced a temperature rise of six degrees Celcius. If she doubles the volume of acid and base she used (while not changing the concentrations), would the temperature rise be half of the original AT (3 C), the same as the original AT (6 C) or twice that of the original AT (12 C) ? Justify your answer. 5. List two things that are necessary for an effective collision at the molecular level. 6. List one way a student can increase the rate that his rock salt (magnesium sulfate pieces) reacts with acid.
- Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go downWhich 0.10 M solution would you expect to have the largest [H+]? Multiple Choice HF (Ka = 6.8 x 10-4) HC2H3O2 (Ka = 1.8 x 10-5) HC3H5O2 (Ka = 1.3 x 10-4) HCN (Ka = 4.9 x 10-10) HCOOH (Ka = 1.8 x 10-4)Use the modified H-H shown below to calculate the blood plasma pH under the following conditions: [HCO3-] = 0.022 M and pCO₂ = 46 mmHg. Provide your answer to two decimal places. Do not enter units. Dissociation Constant pH = 6.1 Bicarbonate (mmol/L) HCO 0.03 x PCO₂ CO₂ Solubility Constant CO₂ Partial Pressure (mmHg)
- Which of the following (assuming the same concentration in water) would make a solution with the lowest hydrogen ion concentration? Group of answer choices H2S (Ka= 8.9×10−8) NH4+ (Ka= 5.6 × 10−10) NH3 ( Kb= 1.8 × 10−5) HC2H3O2 (Ka= 1.8×10−5) HClConsider the following data on some weak acids and weak bases: acid base Ка K, name formula name formula -4 6.8 x 10 ethylamine C,H,NH, 6.4× 10 -4 hydrofluoric acid HF HCH,CO2 1.8 ×x 10 CH;N |1.7× 10 -5 acetic acid pyridine 1.7 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М KI choose one 0.1 M NaF choose one 0.1 М C2HsNHзBr choose one 0.1 M C5H5NHCI choose oneConsider the following data on some weak acids and weak bases: acid base K, formula formula name name HCN CH,NH, 4.3 x 10-10 hydrocyanic acid 4.9x 10-10 aniline HCH,CO, 1.8x 10 s methylamine CH, NH, 44 x 104 acetic acid Use this data to rank the following salutions in order of increasing pH. In other words, select a 'l'next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution p 0.1 M CH,NH,a choose one 0.1 M NaCH,CO2 choose oneY 0.1 M NaNO, choose one 0.1 M KCN choose one
- A chemist prepared aqueous solutions of two weak acids: solution A is hydrazoic acid (HN3), and solution B is propanoic acid (HC2H5CO2). At 25°C, the acid-dissociation constant (Ka) for hydrazoic acid is 2.5x 10-5 and the base-dissociation constant (Kb) for the propanoate ion (C2H5CO2) is 7.8 x 10-10, Determine the following. (a) the Ka value for propanoic acid (HC2H5CO₂) (b) the Kы value for the azide ion (N3) (c) the stronger acid between hydrazoic acid and propanoic acid hydrazoic acid propanoic acid (d) the stronger base between the azide ion and the propanoate ion azide ion Tutorial propanoate ionWhat is the pH of the solution that is prepared by dissolving 0.8 g of lactic acid (90,08 g/mol, Ka - 1.4 x 10) and 1.3g of sodium lactate (112.06 g/mol) in water and diluted to 1.00 L? Round your caiculated value for pH to two figures to the right of the decimal point.Consider an aqueous solution of NaC2H3O2. Which of the following statements is true? A)C2H3O2- is a weak base and NaC2H3O2 is a weak electrolyte. B)C2H3O2- is a strong base and NaC2H3O2 is a weak electrolyte. C)C2H3O2- is a strong base and NaC2H3O2 is a strong electrolyte. D)C2H3O2- is a weak base and NaC2H3O2 is a strong electrolyte.