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for this acid, why does the white bad represent ?

If the pH of the blood of most animals shifts 0.3 units. above or below. the normal range (7.3-7.5), what is going to happen?

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

Ver Historial Favoritos Perfiles Pestaña Ventana Ayuda - Ultra EExperiment 7 - Google Docs G If the pH of a solution is measu X m/document/d/1HGxPrB1Rldlte19cxRUUI2Hoyd-VGYvpF2uipe950iE/edit Format Tools Add-ons Help Last edit was 3 minutes ago Normal text Arial 11 + BIUA 1 | ... 4. 7 C. Effect of Acids and Bases on the pH of a Buffer Solution C1. Effect of an acid on the pH of a buffer solution pH after adding 5 pH after adding Is the tested solution a Initial pH Solution Used Change in pH drops of HCI additional 5 drops of HCI buffer? Yes or No water 6.98 4.05 2.54 2.88 1.95 0.1 M KCI solution 6.40 pH 12 buffer solution 11.98 11.97 11.54 pH 1 buffer solution 2.05 1.85 1.63 C2. Effect of a base on the pH of a buffer solution Solution Initial pH pH after pH after Change in Is the tested

A diprotic acid (H2AH2A) has p?apKa values of 4.934.93 (p?a1pKa1) and 9.869.86 (p?a2pKa2). Which of the equalities is true when the pH is 4.934.93? [HA−]=[A2–][HA−]=[A2–] [H2A]=[A2–][H2A]=[A2–] [H2A]=[HA−][H2A]=[HA−] Which of the equalities is true when the pH is 9.869.86? [H2A]=[A2–][H2A]=[A2–] [HA−]=[A2–][HA−]=[A2–] [H2A]=[HA−][H2A]=[HA−] What is the predominant species of H2AH2A at pH 2.962.96? A2−A2− HA−HA− H2AH2A What is the predominant species of H2AH2A at pH 8.238.23? HA−HA− H2AH2A A2−A2− What is the predominant species of H2AH2A at pH 12.3312.33? A2−A2− HA−HA− H2A

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The pKa of acetic acid, HC2H3O2 is 4.58. A buffer solution was made using an unspecified amount of acetic acid and 0.4 moles of NaC2H3O2 in enough water to make 1.87 liters of solution. It's pH was measured as 3.11. How many moles of HC2H3O2 were used? Report answer with 2 places past the decimal point.

Below is a representation of lysine with three incomplete functional groups in dashed boxes labeled A, B, and C. From the drop down menus choose the correct form of each chemical group that completes the structure of lysine at a neutral pH. COO BN-CH2-CH2-CH2-CH2-C-H N: A A [ Select ] B [ Select] C [ Select] > > >

CaCO3 + 2HCl = CO2 + H2O + CaCl2 How many moles of carbon dioxide gas (CO2) will be produced when the antiacid and your stomach acid react? First you need to calculate the total number of moles of HCl in your stomach (Remember that the volume is 500 mL and use the round up number of the pH question).   The antacid is CaCO3 and the stomach acid is 2HCl.

If the pKa of the indicator is approximately 6, to which of the following equivalence point will it be most suitable?   pH 5   pH 10   pH 4   pH 13

of 13 > A diprotic base (B) has pKg values of 3.33 (pKp1) and 6.66 (pKp2). Which of the equalities is true when the pH is 7.34? Which of the equalities is true when the pH is 10.67? [BH*] = [B] (BH? *) = [BH*) %3D %3D (BH *) = [BH*] O (BH? *1 = [B] [BH? *] = [B] %3D [BH*] = [B] %3! !! What is the predominant species of B at pH 4.40? What is the predominant species of B at pH 9.18? BH? BH? BH* BH+ What is the predominant species of B at pH 12.80? BH? BH

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If the pKa of HCHO 2 is 5.74 and the pH of an HCHO 2/NaCHO 2 solution is 6.11, which of the following is TRUE?   a [HCHO2] >> [NaCHO2]   b [HCHO2] > [NaCHO2]   c [HCHO2] < [NaCHO2]   d [HCHO2] = [NaCHO2]

Boxes 1-4  box 1 answer choices : volume at 1/2 the equivalence point, pH at the equivalence point, pH at the 1/2 equivalence point, initial pH, or volume at the equivalence point. box 2 answer choices: volume at 1/2 the equivalence point, pH at the equivalence point, pH at the 1/2 equivalence point, initial pH, or volume at the equivalence point. box 3 answer choices: volume at 1/2 the equivalence point, pH at the equivalence point, pH at the 1/2 equivalence point, initial pH, or volume at the equivalence point. box 4 answer choices: volume at 1/2 the equivalence point, pH at the equivalence point, pH at the 1/2 equivalence point, initial pH, or volume at the equivalence point.

Experiment : You took 0.51 g of an unknown weak organic acid and dissolved it in 50. ml of water. Then titrated the solution with 0.100 M NAOH and measured the pH after adding 5.00 ml increments of the base, and collected the following data. NaOH (ml) PH 0.0 2.45 5.0 2.95 10.0 3.92 15.0 4.05 20.0 4.35 25.0 8.10 35.0 12.01 40.0 12.20 45.0 12.50 50.0 12.8

Table: Name: Serine      pka: 2.187 (CO2H) / 9.209 (NH3)        Ka: 6.50*10^-3 (CO2H) / 6.18*10^-10 (NH3)   What is the pH, along with the concentration of each form of serine, in a 0.020 0 M solution of serine hydrochloride? What is the pH, along with the concentration of each form of serine, in a 0.020 0 M solution of the sodium salt of serine?  What is the pH, along with the concentration of each form of serine, in a 0.020 0 M solution of serine?  Calculate the isoionic and isoelectric pH for 0.020 0 M serine.

pka=pH halfway to the equivalence point. what is the equivalence point volume? it says to do so by locating the inflection point of the curve. but i'm not sure what the inflection point of the curve is. it says: using a ruler, draw a vertical line that crosses the inflection point and extend this line so it crosses the horizontal axis (use vertical minor gridlines to guide vertical ruler) to find volume base at the equivalence point.

pka=pH halfway to the equivalence point. what is the equivalence point volume? it says to do so by locating the inflection point of the curve. but i'm not sure what the inflection point of the curve is. it says: using a ruler, draw a vertical line that crosses the inflection point and extend this line so it crosses the horizontal axis (use vertical minor gridlines to guide vertical ruler) to find volume base at the equivalence point.

pka=pH halfway to the equivalence point. what is the equivalence point volume? it says to do so by locating the inflection point of the curve. but i'm not sure what the inflection point of the curve is. it says: using a ruler, draw a vertical line that crosses the inflection point and extend this line so it crosses the horizontal axis (use vertical minor gridlines to guide vertical ruler) to find volume base at the equivalence point.

Place each compound into the appropriate category, based on how the compounds behave in water. Strong acid lead chloride PbCl₂ ammonia NH, acetic acid CH,COOH Strong base calcium carbonate CaCO hydrochloric acid HCI Weak acid potassium hydroxide KOH calcium hydroxide Ca(OH), Weak base Answer Bank nitric acid HNO, Soluble salt carbonic acid H₂CO, calcium chloride CaCl₂ Sparingly soluble salt silver nitrate AgNO, magnesium carbonate MgCO,

ll Verizon LTE 12:36 PM O 29% O Question 3 of 16 Submit The pH for 0.0715 M solution of CCl;CO2H is 1.40. Determine the value of Ka for CCl,CO2H. 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Cl,CO,H(a q) H20(1) = H3O*(aq) + CCl,CO; (aq Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0715 1.40 -1.40 0.040 -0.040 0.032 -0.032 +x -x 0.0715 + x 0.0715 - x 1.40 + x 1.40 - x 0.040 + x 0.0340 - x 0.032 + x 0.032 - x

Part A After Larry had taken Nexium for 4 weeks, the pH in his stomach was raised to 4 57. What is the HaO+) in his stomach? Express the concentration to two significant figures and include the appropriate units. H,O*] = Value Units Submit Previous Answers Request Answer X Incorrect; Try Again

PEW41L216q47fR9EANXYnmJnqrAsUafoA6oj JhzTEL52w13Gy9w6bzhg%253D%253D?gameType=async This citrus fruit commonly consumed at home has a ph level of F7 DELL F8 F9 above 7 0 F10 F11 O F12 Exit session 2309 3139 [] Back Oct 26 11:18 0 PrtScr Insert (p Next Delete

Draw a pC-pH diagram for a monoprotic acid with a Ka = 103 M and CTA = 102.5 M. %3D At what pH is the concentration of protonated acid (HA) is 100x greater than the concentration of the conjugate base [A ]? At what pH is the concentration of protonated acid (HA) is 100x greater than the concentration of hydroxide ion [HO`]? Enter your answer as X.X

The image below describes data collected with a pH indicator paper. Identify each sample as acidic, basic or neutral %3D HA Baking Soda" Gastric Juice Black Baking Soda Bleach Coffee Baking Soda 1. Acidic Black Coffee 2. Basic Bleach 3. Neutral Gastric Juice tv >