Module Seven Lesson One Activity (7)

From the National Oceanic and Atmospheric Administration graph about ocean pH above, the following conclusions can be made A. As dissolved carbon dioxide increases, pH becomes more acidic B. As dissolved carbon dioxide increases, pH becomes more basic C. As pH becomes more acidic, dissolved carbon dioxide increases D. As pH becomes more basic, dissolved carbon dioxide decreases

Syl... A solution initial components B C Gr... D O ACIDS AND BASES Making qualitative estimates of pH change Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. . Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. . Use the fifth column to predict how the change in the solution will change its pH. H2O, KOH Explanation H₂O H2O, KOH We... H₂O Check O 14.... OO initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add HClO4 add NaOH add K C104 add Nal 14.... X X effect of change on pH (check one) ООС 0 0 0/0 О С www-awu.aleks A ALEKS-... 27 pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower OpH the same pH higher pH lower pH the same S n Ⓡ tv MacBook Ai

An aqueous solution contains 0.393 M hydrofluoric acid. Calculate the pH of the solution after the addition of 2.07x102 moles of sodium hydroxide to 150 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH = Use the References to access important values if needed for this question. Submit Answer Retry Entire Group 8 more group attempts remaining Previous Email Instructor Next Save and

The table below shows the tolerance of different species in a body of water. Critical pH Levels for Aquatic Organisms Animal Critical pH Level Snails 9. Clams 6. Bass 5.5 Crayfishes 5.5 Mayflies 5.5 Trout Salamanders Perch 4.5 Frogs 4. Source: U.S. EPA Using the data from the table above, which of the following statements best identifies and describes the organism or organisms with the smallest tolérance range to a change in pH in an aquatic environment?

U.S., Find A Grave I.. ? Flowers for Doris G.. Jamie Banks - Unso... Paraphrasing Tool . Com Question 2 20 Only give the exponent including sign for scientific notation. pH: [H*]: РОН: 3 [ОН ]: Question 3

Calculate the pH and the Ka for HC₂H3O2 if in a 1.0000 M solution of HC₂H3O2 in water there is 0.9960 M HC₂H3O2. Use the data provided. HC₂H3O2 + H₂O C₂H30₂¹ + H3O+1 start: 1.00000 M 0 equil: 0.99600 M 0.0040 M 0.0040 M 0.00400 M M. The amount of HC₂H3O2 that was converted into product is mol of C₂H30₂1 and The stoichiometry tells us that 1 mol HC₂H3O2 will give us mol of H30+1 Thus, M HC₂H3O2 will give M H30+1 Because we know the [H3O+¹] we can calculate the pH = -log( [ I ][ [ ] )( c. 0.0040 Ka ( Ka = a. acetic h. CaCO3(s) -1 0. H₂PO4-¹ v. H₂CO3 bb. 0.0077 ii. 1.60 x 10-5 b. 0.9960 i. OH-1 -2 -3 p. CO3-² W. PO4³ CC. 3 jj. 2.398 j. H30+1 q. HCO3-1 x. HC₂H3O2 dd. 2 d. Al+3 kk. 0.05656 K. SO4² r. H₂S y. C₂H30₂-1 ee. 1 e. CO₂ I. Mg+2 S. HS-1 ff. 0.0154 f. CaF2(aq) m. Cl-1 t. S-2 z. 1 x 10-14 gg. 3.95 x 10-3 M C₂H30₂¹ and |) = g. HF(aq) n. HPO4² u. H₂O(liq) aa. 0.9923 hh. 1.84 x 10-6 ii

11. Please answer and show all work, thank you so much!!:)

The hydronium ion concentration in an aqueous solution at 25°C is 7.0x10-2 M. The hydroxide ion concentration is The pH of this solution is The pOH is Submit Answer Use the References to access imp Try Another Version M. 9 item attempts remaining Cengage Learning | Cengage Technical

7 A 0.336 M solution of an acid, HA, has a pH = 2.85. What is the value of the ionization constant K, for this acid? Report your answer with scientific notation with 2 places past the decimal point. Use this format for scientific notation: 1.23*10^-1 Type your answer...

Correction: pH=-log[H+] * Chemistry. The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per liter, in the solution, which means that it is a measure of the acidity or basicity of the solution. The letters pH stand for "power of hydrogen", and the numerical value as defined as pH = Very acid corresponds to pH values near 1, Neutral corresponds to a pH near 7 (pure water), and Very basic corresponds to values near 14. If the wine has an approximate hydrogen ion concentration of 5.01×104 , calculate its pH value.

12. What is the pH of a 1.00 molar solution of NaNO2(aq)? The K, for nitrous acid is 7.0 x 104. a. 1.57 b. 3.15 c. 5.42 d. 8.58 e. 10.85

The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial             concentration of the acid if the pKa of the acid 5.74?     A. 0.657 M   B. 0.387 M   C. 0.315 M   D. 0.0576 M   E. 0.274 M

Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete HCI, proteolytic enzyme zymogens, mucin, and intrinsic factor. The pH of gastric juice is acidic, between 1–3. If the pH of gastric juice is 1.1, what is the amount of energy (AG) required for the transport of hydrogen ions from a cell (internal pH of 7.4) into the stomach lumen? Assume that the potential difference across the membrane separating the cell and the interior of the stomach is –60.0 mV (inside of the cell is negative relative to the lumen of the stomach). Assume that the temperature is 37 °C. The Faraday constant is 96.5 kJ/(V-mol) and the gas constant is 8.314 x 10-3 kJ/(mol·K). Express your answer in kilojoules per mole. AG = kJ/mol

Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete HCI, proteolytic enzyme zymogens, mucin, and intrinsic factor. The pH of gastric juice is acidic, between 1–3. If the pH of gastric juice is 1.9, what is the amount of energy (AG) required for the transport of hydrogen ions from a cell (internal pH of 7.4) into the stomach lumen? Assume that the potential difference across the membrane separating the cell and the interior of the stomach is –70.0 mV (inside of the cell is negative relative to the lumen of the stomach). Assume that the temperature is 37 °C. The Faraday constant is 96.5 kJ/(V-mol) and the gas constant is 8.314 x 10-3 kJ/(mol·K). Express your answer in kilojoules per mole. A = 10.68 kJ/mol

Acid HNO3(AQ) HNO₂(AQ) pH of 0.10 mol/L solution 1.0 2.2 1. Nitric acid and nitrous acid are two acids associated with acid deposition. a. Use the information in the table to identify which acid is a strong acid and which is a weak acid. Support your reasoning without the use of a calculation. Answer: b. Support your answer to question 1.a. using a calculation. Answer:

1 3) 10 11 12 13 14 Calculate the pH at 25 °C of a 0.69M solution of potassium acetate (KCH,CO,). Note that acetic acid (HCH,CO,) is a weak acid with a pK, of 4.76. Round your answer to 1 decimal place. alb pH = Submit Assignment Continue MacBook Air トII FIO FI F7 吕0 F6 D00 F4 F5 esc F3 FI F2 & * %

C What Conc E My Home Alabama A Activity Stre O Dashboard tor asignment-take [Review Topics] [References] Use the References to access important values if needed for this question. In the laboratory, a general chemistry student measured the pH of a 0.577 M aqueous solution of hypochlorous acid to be 3.834. Use the information she obtained to determine the K, for this acid. Ka(experiment) = Submit Answer Retry Entire Group 1 more group attempt remaining Previous Next ENG US Home End Insec F12 &

Number 1