Determine the molarity of 70.5% perchloric acid (HClO4) with a density of 1.67 g/mL? Respond with correct significant figures in scientific notation.
A 0.005 L solution of the strong acid HClO4, has a pH of 2.50. Calculate the mass (number of grams) of HClO4 that was used to make the solution.
A 0.3125 g sample of a primary Na2CO3 standard was treated with 40.00 mL of dilute perchloric acid. The solution was boiled to remove Co 2, and thereafter the excess HClO 4 was titrated by recoiling with 10.12 mL of dilute NaOH. In a separate experiment, it was established that 27.43 mL of HClO4 neutralized the NaOH in a 25.00...
Calculate the pH of each of the following strong acid solutions. (a) 0.00438 M HClO4 pH = (b) 0.579 g of HCl in 21.0 L of solution pH = (c) 59.0 mL of 3.90 M HClO4 diluted to 4.50 L pH = (d) a mixture formed by adding 69.0 mL of 0.00809 M HClO4 to 78.0 mL of 0.00483 M...
Calculate the pH of each of the following strong acid solutions. (a) 0.00471 M HClO4 pH = (b) 0.329 g of HBr in 16.0 L of solution pH = (c) 65.0 mL of 7.50 M HClO4 diluted to 4.60 L pH = (d) a mixture formed by adding 54.0 mL of 0.00155 M HClO4 to 47.0 mL of 0.00191 M...
A) A solution of HClO4 has a pH of 2.41. How many grams of HClO4 are there in 254 mL of this solution? B) How many grams of HClO4 are in 254 mL of. HClO4 solution that has twice the pH?
Write the balanced equations (all three types) for the reactions that occur when the following aqueous solutions are mixed. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) molecular equation: complete ionic equation: net ionic equation: (a)perchloric acid [HClO4(aq)] and iron(III) hydroxide. (b) ammonia (aqueous) and hydroiodic acid. (c) calcium hydroxide (aqueous) and hydrochloric acid....
Hello, is my answer correct for the following Question 1 (1 point) Saved To connect a salt bridge in Dr Musgrove's lab, she had to create a junction between a solution of saturated KCl from the reference electrode (approximately 4.2 M) and a 100. mM solution of perchloric acid (HCLO4) electrolyte. If these solutions were allowed to mix in the...
Consider the titration of 50.0ml of 0.300 M NaOH by 0.100 M HClO4-. Calculate the pH of the solution at the following points in the titration: a) no HClO4 added b) 50.0ml of HClO4 added c) 100.0ml of HClO4 added d) 150.0ml of HClO4 added e) 200.0ml of HClO4 added
Calculate the pH of each of the following strong acid solutions. (a) 0.00890 M HI pH = (b) 0.901 g of HClO4 in 28.0 L of solution pH = (c) 17.0 mL of 3.70 M HI diluted to 4.70 L pH = (d) a mixture formed by adding 12.0 mL of 0.00655 M HI to 72.0 mL of 0.000920 M...