What is the molarity of a KMnO4 solution if the endpoint was reached after pouring 20.55 mL of KMnO4 into 20.00 mL of H2C2O4 solution (conc = 0.0505 M)?

You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.8067 M NaOH and the equivalence point is reached by the addition of 17.31 mL of NaOH solution.  Using the balanced equation below, calculate the molartity of H2SO4 in the flask. Do NOT include units.  2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)

how do i find molarity of diluted KMnO4 solution if the molarity of stock KMnO4 is 0.0200M and a 100ml volumetric flask was filled with 5.00ml of KMnO4 and the rest with water?

What volume of acid with a concentration of 0.0010 M is needed to neutralize 0.695 g of CaCO3 in the following reaction:  CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)

16. How would you set up and solve the mole calculation?

MISSED THIS? Read Section 14.4 (Page); Watch KCV 14.4. A solution contains 29 g of KNO3 per 100.0 g of water at 25 °C. 100 Solubility (g solute in 100 g H₂O) 90 80 70- 60- 50 40 30 20 10 0 0 NaNOs Pb(NO3)2 NaCl CaCl₂ T 10 SONX Na₂SO4 KCI KC103 T 20 30 40 50 60 Temperature (°C) 70 80 K₂Cr₂O7 90 100 Part A Is the solution unsaturated, saturated, or supersaturated? (Refer to the figure on the left.) O saturated O supersaturated O unsaturated Submit Request Answer Review Provide Feedback

Question 7 of 10 Submit What volume in L of a 0.724M Nal solution contains 0.405 | mol of Nal ? X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) %3D 0.405 0.293 g Nal L 126.90 g Nal/mol 0.559 mol Nal 559 mL 22.99 M Nal 148.89 6.022 x 1023 1.79 0.724 Tap here or pull up for additional resources

What quantity in moles of precipitate will be formed when 60.5mL of 0.350M AgNO3 is reacted with excess Mgl2 in the following reaction? 2 AgNO3(aq)+Mgl2(aq)= 2Agl(s)+Mg(NO3)2(aq)

o A chemist wants to extract a solute from 100 mL of water using only 300 mL of ether. The distribution constant, Kp, between ether and water is 1.99. Calculate q, the fraction of solute that would remain in the water under each of the extraction conditions. The chemist performs a single extraction with 300 mL of ether. 9 = The chemist performs three extractions with 100 mL of ether. 9= The chemist performs six extractions with 50 mL of ether. 9 =

The boiling point of diethyl ether, CH3CH₂OCH₂CH3, is 34.500 °C at 1 atmosphere. Kö(diethyl ether) 2.02 °C/m In a laboratory experiment, students synthesized a new compound and found that when 11.39 grams of the compound were dissolved in 297.6 grams of diethyl ether, the solution began to boil at 34.768 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? g/mol