3. pH is a measure of the concentration of water molecules that have dissociated into ions. This number is very small, so very, very small that it is annoying as ^%$@#% to write out. Therefore, we convert this by equation to a measure of "pH" to make is easier to describe the level of ionization. It is a characteristic of water that the product of the concentration of each ion of water will equal 10¹4 (i.e. in aqueous solutions, [ H+] x [OH-] = 10", where [] is used to represent concentration in moles/liter). a. We can write that several ways (fill in the missing parts): 10¹4 = 10^-14 = 1/10^ = 1 in b. At neutral pH, the concentration of H+ = 10^-7. But we all hate exponents, especially negative exponents, so we use this equation to make a pretty pH number pH=-log [H+]. pH = -log[ 10^-7] = (review the Bioskills appendix to practice using
3. pH is a measure of the concentration of water molecules that have dissociated into ions. This number is very small, so very, very small that it is annoying as ^%$@#% to write out. Therefore, we convert this by equation to a measure of "pH" to make is easier to describe the level of ionization. It is a characteristic of water that the product of the concentration of each ion of water will equal 10¹4 (i.e. in aqueous solutions, [ H+] x [OH-] = 10", where [] is used to represent concentration in moles/liter). a. We can write that several ways (fill in the missing parts): 10¹4 = 10^-14 = 1/10^ = 1 in b. At neutral pH, the concentration of H+ = 10^-7. But we all hate exponents, especially negative exponents, so we use this equation to make a pretty pH number pH=-log [H+]. pH = -log[ 10^-7] = (review the Bioskills appendix to practice using
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Understanding pH and Ion Concentration**
**3. pH Explained:**
pH is a measure of the concentration of water molecules that have dissociated into ions. This number is very small, so small that it becomes cumbersome to write out. Therefore, it is converted to a measure of "pH" to make it easier to describe the level of ionization.
**Ion Concentration of Water:**
In water, the product of the concentration of each ion will equal \(10^{-14}\). In aqueous solutions, \([H^+][OH^-] = 10^{-14}\), where brackets \([]\) denote concentration in moles/liter.
**Exercises:**
**a. Writing Exponents:**
\[ 10^{-14} = 10^{-14} = \frac{1}{10^7} \times \frac{1}{10^7} = 1 \]
\[ 1 \text{ in } 10^7 \text{ solutions } \]
**b. Neutral pH:**
At neutral pH, the concentration of \([H^+] = 10^{-7}\). To simplify exponents, especially negatives, use the equation:
\[ \text{pH} = -\log [10^{-7}] = \underline{\quad} \]
(Review the Bioskills appendix for practice with logarithmic functions.)
**c. Neutral pH Conditions:**
If pH = 7, then \([10^{-7}] \times [OH^-] = 10^{-14}\), so \([OH^-] = \underline{\quad}\)
**d. Calculating pH for Different \([H^+]\):**
If \([H^+] = 10^{-9}\), then pH = \underline{\quad}
**e. Relationship of \([H^+]\) and pH:**
As \([H^+]\) increases, the pH \underline{\quad}
**Note:**
\[ x^a \times x^b = x^{(a+b)} = x^c \]
This section provides an understanding of how pH is determined and how it relates to ion concentration in solutions. Use logarithmic calculations to simplify and express these relationships effectively.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F087af6b6-013e-4f7d-bfdc-f2223ece6aff%2Fdec88266-9331-46eb-991a-49d177494e84%2F5oe0wbi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Understanding pH and Ion Concentration**
**3. pH Explained:**
pH is a measure of the concentration of water molecules that have dissociated into ions. This number is very small, so small that it becomes cumbersome to write out. Therefore, it is converted to a measure of "pH" to make it easier to describe the level of ionization.
**Ion Concentration of Water:**
In water, the product of the concentration of each ion will equal \(10^{-14}\). In aqueous solutions, \([H^+][OH^-] = 10^{-14}\), where brackets \([]\) denote concentration in moles/liter.
**Exercises:**
**a. Writing Exponents:**
\[ 10^{-14} = 10^{-14} = \frac{1}{10^7} \times \frac{1}{10^7} = 1 \]
\[ 1 \text{ in } 10^7 \text{ solutions } \]
**b. Neutral pH:**
At neutral pH, the concentration of \([H^+] = 10^{-7}\). To simplify exponents, especially negatives, use the equation:
\[ \text{pH} = -\log [10^{-7}] = \underline{\quad} \]
(Review the Bioskills appendix for practice with logarithmic functions.)
**c. Neutral pH Conditions:**
If pH = 7, then \([10^{-7}] \times [OH^-] = 10^{-14}\), so \([OH^-] = \underline{\quad}\)
**d. Calculating pH for Different \([H^+]\):**
If \([H^+] = 10^{-9}\), then pH = \underline{\quad}
**e. Relationship of \([H^+]\) and pH:**
As \([H^+]\) increases, the pH \underline{\quad}
**Note:**
\[ x^a \times x^b = x^{(a+b)} = x^c \]
This section provides an understanding of how pH is determined and how it relates to ion concentration in solutions. Use logarithmic calculations to simplify and express these relationships effectively.
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