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Acids & Bases Chapter 14A

Understand the characteristics and interactions of acids and bases, including pH scales, neutralization reactions, and Bronsted-Lowry definitions. Explore how these substances change indicator colors and their impact on solutions. Gain insights into the Arrhenius theory and pH measurement techniques. Enhance your knowledge on the properties of common acids and bases.

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Acids & Bases Chapter 14A

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  1. Acids & BasesChapter 14A West Valley High School General Chemistry Mr. Mata

  2. Standard 5C • Students will know the observable properties of acids, bases, & salts.

  3. Essential Question: What are the general properties of acids and bases?

  4. PROPERTIES OF ACIDS • General formula of acid is HX. • Sour taste; corrosive; contain H +1 (hydrogen ions). • Aqueous solutions are electrolytes. • Cause indicators to change color: • BLUE LITMUS PAPER + ACID -> RED COLOR • React with some metals to produce H2(g). • React with bases to produce salt & water. • pH = 0 to 6.9999 on pH scale. • Ex: vinegar, citrus fruits

  5. Properties of Bases • General formula XOH (where X is a metal). • Taste bitter; corrosive; OH -1 (hydroxide ions). • Feel slippery to touch. • Cause indicators to change color: • RED LITMUS PAPER + BASE ->BLUE COLOR • Aqueous solutions are electrolytes. • React with acids to produce salt and water. • pH = 7.0001 – 14 on pH scale. • Ex: ammonia, lye

  6. Neutralization Reaction • Acid +Base->Salt + Water • ex: HCl + NaOH -> NaCl + H2O • H + 1 ion combines with OH -1 ion -> H2O. • Na +1 ion combines with Cl -1 ion -> NaCl. • H2O is neutral with pH = 7.000

  7. Arrhenius Acids and Bases • Svante Arrhenius (1884) proposed theory of ionization for acids & bases. • Definition - Acids release hydrogen ions (H +1). - Bases release hydroxide ions (OH -1).

  8. Arrhenius Acids and Bases • Acids may be mono, di, or triprotic. • Nitric acid (HNO3) = ? H +1 ion • 1 H +1 ion = monoprotic acid • Sulfuric acid (H2SO4) = ? H +1 ion • 2 H +1 ions = diprotic acid • Phosphoric acid (H3PO4) = ? H +1 ion • 3 H +1 ions = triprotic acid

  9. Bronsted-Lowry Acids and Bases • Bronsted-Lowry acid = H +1 ion donor. • Bronsted-Lowry base = H +1 ion acceptor. H +1 • Ex: H2O + NH3 -> OH -1 + NH4+1 acid base

  10. Meaning of pH • pH = “power of hydrogen”. • Acids have pH from 0 to 6.9999. • A neutral solution has a pH of 7.0000 • Bases have pH from 7.0001 to 14. • pH + pOH = 14 • “[ ]” = concentration or molarity • [H+ 1] x [OH- 1] = 1 x 10 -14 M

  11. The pH Concept • Express large [H+ 1] ion concentrations using smaller numbers. • Logrithmic scale (base 10 units). • pH = - log [H+ 1] • [H+] = 1 x 10 –3 M -> pH = 3 (acidic) • [H+] = 1 x 10 –7 M -> pH = 7 (neutral) • [H+] = 1 x 10 –11 M -> pH = 11 (basic)

  12. The pH Scale • 1 pH unit change = 10x change • pH > 7 basic • pH = 7 neutral • pH < 7 acidic

  13. Measuring pH • Variety of different indicators. • Indicators are acids or bases that change color with the changing [H+1]. • Phenol Red (swimming pools) and phenolphthalein (trace blood). • Can use pH meter, litmus paper (red or blue), pH paper.

  14. Chapter 14A SUTW Prompt • Describe how acids and bases are organized on the pH scale. • Complete a 8 -10 sentence paragraph using the SUTW paragraph format. Hilight using green, yellow, and pink. • Due Date: Monday, February 5, 2018 (start of class).

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