If lime juice has a pH of 1.7, what is the concentration of hydrogen ions (in [tex]$mol / L$[/tex]) in lime juice, to the nearest hundredth? Use the formula [tex]$pH=-\log [H+]$[/tex].
Answer (2)
Substitute the given pH value into the formula: 1.7 = − lo g [ H + ] .
Multiply both sides by -1: − 1.7 = lo g [ H + ] .
Take the antilog (base 10) of both sides: [ H + ] = 1 0 − 1.7 .
Calculate the value and round to the nearest hundredth: [ H + ] ≈ 0.02 .
The concentration of hydrogen ions is 0.02
Explanation
Problem Analysis We are given that the pH of lime juice is 1.7 and the formula relating pH to the concentration of hydrogen ions [ H + ] is p H = − lo g [ H + ] . We need to find the concentration of hydrogen ions in m o l / L to the nearest hundredth.
Substitute pH value Substitute the given pH value into the formula: 1.7 = − lo g [ H + ]
Multiply by -1 Multiply both sides of the equation by -1: − 1.7 = lo g [ H + ]
Take antilog Take the antilog (base 10) of both sides to solve for [ H + ] : [ H + ] = 1 0 − 1.7
Calculate and round Calculate the value of 1 0 − 1.7 . The result of this operation is approximately 0.01995. Rounding this to the nearest hundredth gives us 0.02.
Final Answer Therefore, the concentration of hydrogen ions in lime juice is approximately 0.02 m o l / L .
Examples
Understanding pH and concentration of hydrogen ions is crucial in many real-world applications. For example, in agriculture, knowing the pH of the soil helps farmers determine the best crops to grow and the necessary soil treatments. In medicine, maintaining the correct pH balance in the body is essential for various biological processes. In environmental science, monitoring the pH of water sources helps assess water quality and the impact of pollutants. The formula p H = − lo g [ H + ] allows us to quantify the acidity or alkalinity of a substance, providing valuable information for informed decision-making in these fields.
The concentration of hydrogen ions in lime juice with a pH of 1.7 is approximately 0.02 mol/L. This is calculated using the formula pH = -log[H+]. After substituting the pH value and solving, we find that [H+] rounds to 0.02 mol/L.
;
