Page 16: Draw a picture of a pH scale. Be sure to label the following terms or your picture: acid, base, neutral, high concentration of hydrogen (H*), & low concentration of hydrogen (H¹).
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- Which of the following combinations would be the best choice to buffer the pH of a solution at approximately 7? Ionization Constants for Aqueous Weak Acids at 25 °C Acid K. (pK,) Conjugate Base Hydrogen phthalate ion, Cg H4(CO2H)(CO2) Acetic acid, CH3 CO,H Acetate ion, CH; CO2- 1.8 x 10-5 (4.74) Weak Acid Phthalic acid, C6 H4 (CO,H)2 1.3 x 10-3 (2.89) Dihydrogen phosphate Hydrogen phosphate ion, H2 PO4 Hydrogen phosphate ion, HPO42 6.2 x 10-8 (7.21) ion, HPO,2- Phosphate ion, PO,* 3.6 x 10-13 (12.44) O Na, HPO4 and NagPO4 O NaH2 PO4 and NazHPO4 O H;PO4 and NaH2 PO4pH with 0 mL of pH with 5 mL of pH with 10 mL of Cola Buffer pH with 20 mL Cola Cola of Cola Buffer F 4.5 4.8 4.1 4.4 Buffer H (water) |7.0 3.2 n/a n/a Is Buffer F (the acetic acid - sodium acetate buffer you made) a good buffering system for acids? Explain your reasoning.discuss any complications of acidity or alkalinity of foods on another organ or system in the body? How do acids and base relate to your working environment? (For instance, you could consider the chemicals in a cleaning solution.) Solve it asap
- pH: Acids and Bases Name: 15. An acid is called an acid because of the amount of positive hydrogen ions that are dissolved in the solution. Based en this concept, which substance has more hydrogen ions dissolved in the solution? (circle one for each) a Vomit b. Hand soap c. Blood or chicken soup drain cleaner soda or or 16. A base is called a base because of the amount of hydroxide lons that are dissolved in the solution. Based on this concept, which substance has more hydroxide ions dissolved im the solution? (circle one for each) a. Milk b Blood c. soda pop spit coffee or or battery acid or Test your understanding and self check muT ad nnort your anver with an explanation. Then use pH ScaleDefine the term buffer. Explain the difference between carbonic acid (H2CO3) and hydrochloric acid (HCl). Can they both be used as buffers? Why or why not.A buffer solution is composed of 1.00 mol of acid and 1.75 mol of the conjugate base. If the pKa of the acid is 3.60, what is the pH of the buffer? pH=
- Based on the pH of your drug, if your drug was in a high concentration in the blood, how would it affect the pH of your blood. Would it cause acidosis or alkalosis, and how would you treat this? the drug name is captopril and the pH is 2.65Describe the pH scale and the role of buffers in body fluids.The pHpH scale for acidity is defined by pH=−log10[H+] where [H+]is the concentration of hydrogen ions measured in moles per liter (M). A solution has a pH of 10.2. Calculate the concentration of hydrogen ions in moles per liter (M).
- Define the terms acidic, basic, acid, and base. Also define pH and describe the relationship between pH and the H+ concentration of a solution.Complete the table below. Assume that the only reaction is dissolution. Ignore the effects of acid/base hydrolysis. Show complete solutions. Show both the rounded and non-rounded answers. For the rounded answer, express in exactly 5 significant figures. Salt Ksp Common ion [cation] [anion] AgX 2.24 х 103 М х 5.27 х 109м Hg2X2 1.33 x 102 M Hg2* 1.65 x 107 MA solution has a hydrogen ion concentration of 0.01 mol/L. What is its pH? What is its hydroxide ion concentration? Is it acidic, basic, or neutral? How does the hydrogen ion concentration of this solution differ from one with a pH of 1?