- Write the balanced equation for the hydration of  CuSO4. Indicate the physical states using the abbreviations ( s ), (l), (g)or solid, liquid, or gas, respectively. Use ( aq ) to indicate the aqueous phase. Indicate appropriate charges on negative and positive ions if they are formed. Express your answer as a complete chemical equation including all phases. Do not include water in your answer.     - How many milliliters of a 7.150 MM HClHCl solution are required to react with 34.30 gg magnesium?

Suppose 37.3 g of ammonium iodide is dissolved in 300. mL of a 0.60 M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the ammonium iodide is dissolved in it. Be sure your answer has the correct number of significant digits.

Balance the following chemical reaction. Enter the sum of the balanced coefficients as your answer. Assign "blank" coefficients a value of 1. silver iodide + sodium sulfide → silver sul fide + sodium iodide

Answer the following question: How many moles of ammonia are in 500. ml of a 2.25 M aqueous ammonia solution? Find the numerical answer for this question and make sure to include the following: • What is the chemical formula for ammonia? • What is the formula for molarity? • When you give your numerical answer, what is the correct significant figures and how do you know that is the correct amount?

Suppose 20.4 g of ammonium sulfate is dissolved in 150. mL of a 0.70 M aqueous solution of sodium chromate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume of the solution doesn't change when the ammonium sulfate is dissolved in it. Be sure your answer has the correct number of significant digits.

For the following, use proper sig figs, do not include units, and do not place numbers in scientific notation. A simple equation that can be used ONLY for dilutions is M1V1 = M2V2. So if a concentrated solution starts out as 1.36 M and you wish to make 50.0 mL of a 0.286 M solution, how many milliliters of the concentrated solution do you need? How much water will you add?

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.

[Review Topics] [References] Use the References to access important values if needed for this question. For the following reaction, 136 grams of perchloric acid (HCIO4) are allowed to react with 25.6 grams of tetraphosphorus decaoxide. perchloric acid (HClO4) (aq) + tetraphosphorus decaoxide(s) → phosphoric acid (aq) + dichlorine heptaoxide (1) What is the maximum amount of phosphoric acid that can be formed? Mass= g What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? Mass= g Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous Next> Save and Exit

Sodium carbonate is used in toothpaste where it acts as a foaming agent and an abrasive. Calculate the mass (in grams) of solute needed to prepare 53 mL of a 0.443 mol/L solution of Na2CO3   Record only your numerical answer with the correct number of significant digits.  You do not need to include units as the units appear for you beside the answer box already.

Suppose 3.23 g of iron(II) iodide is dissolved in 50. mL of a 0.20 M aqueous solution of silver nitrate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the iron(II) iodide is dissolved in it. Round your answer to 2 significant digits.