Prepare 250mL of a 0.75M solution of phosphoric acid from 75.0% phosphoric acid that is pure. The gram formula weight of phosphoric acid is 98.00 g/mol, and the density of 75.0% phosphoric acid is 1.58g/mL

Please answer the question! Find the molarity and mass percent of ammonium hydroxide solutions. Thanks!

Consider the reaction between 50.0 mL of 0.10 M NaOH and 75.0 mL of 0.20 M HCI at 25°. Which of the following statements is TRUE? HCl is the limiting reactant. After the reaction, the concentration of Na* is equal to the concentration of Cl'. After the reaction, the concentration of Cl' is still 0.200 M because Cl' is a spectator ion. After the reaction, the concentration of Na* is greater than the concentration of H30*. The final solution has a pH 1.10.

Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Be sure each entry you write includes the correct number of significant digits. [1,0"] solution pH x10 olo -8 A 1.5 X 10 mol/L Ar В ||mol/L 2.24 - 11 mol/L 2.1 X 10 C

To best accurately determine the molarity of a base, a scientist would need the following: An Erlenmeyer flask, a weighed solid primary standard acid, and NaOH A buret, a weighed solid monobasic base, and an indicator A buret, a weighed solid primary standard acid, and an indicator A buret, a weighed solid primary standard acid, and NaOH A graduated cylinder, a weighed solid primary standard acid, and an indicator

What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M?    A 34.1 % (NH4 )2SO4   (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution?  (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)     Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)   NEED HELP ASAP NO WORK NEEDED

the percentage of KHP in an unknown sample was determined. Which of the following is NOT true. Aqueous NaOH should be standardized so concentration is accurately known. The moles of KHP can be determined at the endpoint, which is close to the equivalence point. Percentage of KHP, is equal to the mass of KHP found, divided by the mass of the unknown, multiplied by 100.

Determine the pOH (to two decimal places) of the solution that is produced by mixing 2.23 mL of 2.32x10-4 M SrH2 with 19.9 mL of 1.80×10-1 M SrO.

Calculate the percent dissociation of benzoic acid (CH₂CO₂H) in a 2.5 mM aqueous solution of the stuff. You may find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. []% x10 X ? Ś

Consider the diagram of an aqueous solution of a soluble ionic compound. 2+ Determine which ionic compound is dissolved 2+ in solution. 2+ KCI 2+ СаBr, MgCrO, Ca(CIO,), C