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What is the pH of a solution that contains 1.2 moles of HNO3 and 1.7 moles of HCL dissolved in 1000 liters of water?
To find the pH, calculate the total moles of H+ ions from the given acids (HNO3 and HCl). The total moles of H+ ions is 1.2 + 1.7 = 2.9 moles. Since the volume is 1000 liters, the concentration of H+ ions is 2.9 moles/1000 liters = 0.0029 M. Finally, calculate the pH using the formula pH = -log[H+]. So, pH = -log(0.0029) = 2.54.
How many moles of H3O are present in an 85 L solution with a pH of 3.0?
To find the number of moles of H3O in the solution, you can use the formula pH -logH3O. First, calculate the concentration of H3O ions using the pH value: pH -logH3O 3.0 -logH3O H3O 10(-3.0) 1.0 x 10(-3) M Next, calculate the number of moles of H3O in the solution using the concentration and volume: moles concentration x volume moles 1.0 x 10(-3) mol/L x 85 L moles 8.5 x 10(-2) moles Therefore, there are 8.5 x 10(-2) moles of H3O present in the 85 L solution with a pH of 3.0.
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
What is the pH of a solution that contains 1.2 moles of nitric acid (HNO3) and 1.7 moles of hydrochloride acid (HCI) dissolved in 1000 liters of water?
To calculate the pH of the solution, first determine the total moles of H+ ions in the solution by adding the moles of H+ ions from both acids. Then, calculate the molarity of the H+ ions in the solution by dividing the total moles by the volume of the solution in liters. Finally, use the formula pH = -log[H+].
What is th unit of measure used to express the concentration of an acid or base?
The concentration of an acid or base is typically expressed in moles per liter (mol/L) or molarity (M).
What is the pH of a solution that contains 1.2 moles of HNO3 and 1.7 moles of HCL dissolved in 1000 liters of water?
To find the pH, calculate the total moles of H+ ions from the given acids (HNO3 and HCl). The total moles of H+ ions is 1.2 + 1.7 = 2.9 moles. Since the volume is 1000 liters, the concentration of H+ ions is 2.9 moles/1000 liters = 0.0029 M. Finally, calculate the pH using the formula pH = -log[H+]. So, pH = -log(0.0029) = 2.54.
When an strong acid and weak base meet What is the pH?
The pH that results when a strong acid and strong base are mixed will depend on the moles of acid and moles of base present. One cannot predict the pH without knowing, or being able to calculate, the moles of each.
How many moles of H3O are present in an 85 L solution with a pH of 3.0?
To find the number of moles of H3O in the solution, you can use the formula pH -logH3O. First, calculate the concentration of H3O ions using the pH value: pH -logH3O 3.0 -logH3O H3O 10(-3.0) 1.0 x 10(-3) M Next, calculate the number of moles of H3O in the solution using the concentration and volume: moles concentration x volume moles 1.0 x 10(-3) mol/L x 85 L moles 8.5 x 10(-2) moles Therefore, there are 8.5 x 10(-2) moles of H3O present in the 85 L solution with a pH of 3.0.
What is it when The number of moles of hydrogen ions equals the number of moles of hydroxide ions?
A neutral solution of about 7 pH.
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
What is the pH of a solution that contains 1.2 moles of nitric acid (HNO3) and 1.7 moles of hydrochloride acid (HCI) dissolved in 1000 liters of water?
To calculate the pH of the solution, first determine the total moles of H+ ions in the solution by adding the moles of H+ ions from both acids. Then, calculate the molarity of the H+ ions in the solution by dividing the total moles by the volume of the solution in liters. Finally, use the formula pH = -log[H+].
Write the equation for determining pH?
pH = -log[H+], where [H+] is the hydrogen ion concentration in moles per liter.
How is pH scale applied to logarithmic equation?
The pH scale is a logarithmic scale used to express the acidity or basicity of a solution. The formula to calculate pH is pH = -log[H+], where [H+] is the hydrogen ion concentration in moles per liter. This logarithmic equation allows for a convenient way to represent a wide range of hydrogen ion concentrations in a compact form.
What is th unit of measure used to express the concentration of an acid or base?
The concentration of an acid or base is typically expressed in moles per liter (mol/L) or molarity (M).
What can the coefficients in a balanced chemical equation always express the ratio of?
Moles of one substance compared to moles of the second substance. Ex. moles of reactant A compared to moles pf product F
What is the approximate pH of the equivalence point in the titration pH curve?
The approximate pH of the equivalence point in a titration pH curve is around 7 for a strong acid-strong base titration. This is because at the equivalence point, the moles of acid are equal to the moles of base, resulting in a neutral solution.
The equivalence point reached when the pH reaches it maximum value?
The equivalence point is reached in a titration when the moles of acid are equal to the moles of base added. At the equivalence point, the pH of the solution is at its maximum or minimum value, depending on whether a strong acid or base is used in the titration.
