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Caves form mostly from the reaction of weak carbonic acid (which forms due to carbon dioxide that is in the water) with exposed limestone. What numbers go in the blanks below, in order from left to right, to balance this chemical equation? ___H2CO3(aq) + ___CaCO3(s) --> ___Ca(HCO3)2(aq) + ___CO2(g) + ___H2O(l)
the vapor pressure of chlorine dioxide clo2 is155torrat-22.75 ? cand485torrat 0?c. what is the normal boiling point of
the enthalpy change when a strong acid is neutralized by strong base is -56.1 kjmol. if 135 ml of 0.450 m hi at
How many moles of NaOH were used? How many moles of H3PO4 were in the cola sample? What is teh concentration of H3PO4 in the cola sample?
What is the molecular equation, total ionic equation, and net ionic equation for Cu(NO3)2 and NaOH
if two atoms of element A react with three atoms of element B, what is the chemical formula for the resulting compound
What is the theoretical yield (in grams) of the precipitate when 22.2 g of iron(II) chloride reacts in solution with 10.91 g sodium hydroxide
In which of the following aqueous solutions would you expect AgCl to have the LOWEST solubility? A. pure H2O, B. 0.020 M BaCl2, C. 0.015 M NaCl, D. 0.020 AgCl
The bold part is my question, as I believe the first part is already correct. Please provide an explanation. Solutions of Cu2+ turn litmus red because of equilibrium for which Ka=1.0e-8. Calculate the pH of 0.10 M Cu(NO3)2.
At 0.0 C, if the volume of air is 2 mL and the pressure of the atmosphere that day is 665 mmHg, what is the number of moles of air?
Define how many grams of the excess reactant are left over according to the reaction below given that you begin with 10.0 g of Al and 19.0 grams of O2
Problem- Consider the titration of 36.6mL of 0.255M HF with 0.180M NaOH. Calculate the pH at each of the following points. Calculate the pH after the addition of 9.15mL of base. Calculate the pH at halfway to the equivalence point.
100 mL of 0.150 M acid HA are mixed with 100 mL of 0.0800 M NaOH. Calculate the titration constant, kt, of the resulting reaction. Ka = 1.0 x 10-5
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