.. A solution of NaOH has a oxalic acid (MW 126.0) titer of 9.45 mg/mL. Calculate the normality of the NaOH solution. (Oxalic acid furnishes two hydrogen ions) Calculate the following titors in ma/ml.

(10 ||| Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Microsoft O Predicting precipitation W Microsoft Microsoft 6.52.210... esc solution A zinc nitrate iron(II) iodide iron(II) nitrate Explanation 5 T C solution B ammonium sulfide zinc nitrate potassium hydroxide Check 9,216 280 #m Does a precipitate form when A and B are mixed? 103 yes NOV 1 yes O yes no $ 4 no no OOO % Q Search or enter website name LO empirical formula of precipitate 5 0 0 stv 6 X & 7 5 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility * 00 8 A ( 9 W 0 DOCX – + 11 { olo Ar 2 lal h Eng

What volume of 2.5 M H3PO4 (aq) would be required to neutralize 2.50 mL of 1.5 M NaOH? НЗРО4 (аq) + 3 NaOH (ag) --> Na3PО4 (aq) + 3 Н20 ()

At 700 deg C (1290\deg F), what is the maximum solubility (a) of Cu in Ag? (b) Of Ag in Cu? .

Determine the number of grams of PbCl2 produced from 100.0 ml of 0.20 M Pb(NO3)2 and sufficient NaCl in the following precipitate reaction  2 NaCl + Pb(NO3)2 --> PbCl2 + 2 Na(NO3)   Could you please solve by filling in the blanks in the image.

Suppose you are given three bottles, labeled A, B, & C; each contains an aqueous solution. You are told that the possible solutions are: sodium hydroxide, nickel(II) chloride, potassium thiocyanate, sodium acetate, and pure water. Only one type of solution is present in each bottle and the con 0.5 M unless otherwise noted. Several tests are performed, and the results are summarized in the flow chart displayed on the right. Based on these results, assign the contents of the bottles and write a brief justification for each assignment. (The type of pH paper you will use is the same as the one described in the chemical foundations section).

Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = M

You mix 275.0 mL of 1.20M Pb(NO3)2 with 300.0 mL of 1.85 M KI. Calculate the mass of precipitate.

The solubility of magnesium fluoride, M&F2, in water is 1.5 x 10- g/L. What is the solubility (in grams per liter) of magnesium fluoride in 0.29 M of sodium fluoride, NaF? Solubility = |g/L

Hydrobromic acid can be purchased as 50.0% solution. The density of this solution is 1.07 g mL-1. What is the molar concentration of hydrobromic acid in this solution? The molar concentration = i M