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Use Kw to calculate concentrations of hydroxide and...
Calculate the concentrations of hydroxide and hydronium ions in a solution prepared by dissolving 0.471 g...
Calculate the concentrations of hydroxide and hydronium ions in a solution prepared by dissolving 0.471 g of solid NaOH in enough water to make 225 mL of solution. Kw = 1.0E-14. Hydroxide ion concentration? M The number of significant digits is set to 3; the tolerance is +/-4% LINK TO TEXT Hydronium ion concentration? M The number of significant digits is set to 3; the tolerance is +/-4%
A sample of carbon dioxide in water at room temperature has a hydroxide ion concentration of...
A sample of carbon dioxide in water at room temperature has a hydroxide ion concentration of 7.9 x 10 hydronium ion concentration of the solution? M. What is the • Your answer should include two significant figures. • Write your answer in scientific notation. Use the multiplication symbol rather than the letter in your answer. Provide your answer below.
ay 24: K Learn objective - The pH and pOH Scales Calculate concentrations of hydronium and...
ay 24: K Learn objective - The pH and pOH Scales Calculate concentrations of hydronium and hydroxide ions Question = 5.13 x 10-13. What is the concentration of hydroxide ions at this At 100 °C, the ion product of water is K temperature? Select the correct answer below: O 2,56 x 10-4 M 0 5.06 x 10- M 7.16 X 10 M There is not enough information
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a...
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a pH of 2.0. Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 2. What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 3. Which is the stronger acid, NH4+ or HBrO? Hint: Compare...
please show work where necessary. 6) Calculate the hydroxide and hydronium ion concentrations for the following...
please show work where necessary.
6) Calculate the hydroxide and hydronium ion concentrations for the following solutions a) pH = 7,0 [H,0") - (OH) = b) pH = 1000 [H,0") - (OH) - 7) From the given value, calculate the other three. Use the figure to take the most efficient pathway possible! a) C) pH 6.5 pH = рон • pOH = [OH- (OH) - 1.6 10-M [H,0") - [H,0"] - b) d) pH pH pOH = 9.8 рона (OH)...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e)...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...
my Nules || Ask Your Teac The concentration of hydroxide ions in an aqueous solution is...
my Nules || Ask Your Teac The concentration of hydroxide ions in an aqueous solution is 3.8x109 M. What is the concentration of hydronium ions in this solution at 25°C? M Need Help? 2. - 3 points WAS OSGENCHEM1 14.1.WA.017. My Notes Ask Your Teache Calculate the concentration of the hydroxide ion (OH) in an aqueous solution if the hydronium ion (H20) concentration is 4.98 x 10 Kw - [H,0*1(OH) - 1.01x10-14 at 25°C. moll mol/L. The lon-product constant for...
Which statements listed below can explain why a chemical reaction does not take place? concentration of...
Which statements listed below can explain why a chemical reaction does not take place? concentration of reactants is too low the temperature is too low not enough effective collisions are occurring some of these answers all of these answers For a chemical reaction the rate of the forward reaction is at a maximum when when the concentration of the reactants and products is the same a state of equilibrium is reached the reaction begins the concentration of products is greater...
3. i). Write the formula of four strong acids and four strong bases. ii). List four...
3. i). Write the formula of four strong acids and four strong bases. ii). List four factors that affect the strength of an acid. iii). Predict the relative strength of the following compounds: H2O, H2S and H2Se. iv). Which of the following is the stronger acids: CHCICOOH or CHCI-COOH? Explain. v). Al 3* is not a Bronsted acid, Al(H2O)" is. Explain. vi). All Bronsted acids are Lewis acids, but the reverse is not true. Give two examples of two Lewis...
1. Which of the followi ch of the following reactions is not readily explained by the...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
A sample of carbon dioxide in water at room temperature has a hydroxide ion concentration of 7.9 x 10 hydronium ion concentration of the solution? M. What is the • Your answer should include two significant figures. • Write your answer in scientific notation. Use the multiplication symbol rather than the letter in your answer. Provide your answer below.
ay 24: K Learn objective - The pH and pOH Scales Calculate concentrations of hydronium and hydroxide ions Question = 5.13 x 10-13. What is the concentration of hydroxide ions at this At 100 °C, the ion product of water is K temperature? Select the correct answer below: O 2,56 x 10-4 M 0 5.06 x 10- M 7.16 X 10 M There is not enough information
please show work where necessary.
6) Calculate the hydroxide and hydronium ion concentrations for the following solutions a) pH = 7,0 [H,0") - (OH) = b) pH = 1000 [H,0") - (OH) - 7) From the given value, calculate the other three. Use the figure to take the most efficient pathway possible! a) C) pH 6.5 pH = рон • pOH = [OH- (OH) - 1.6 10-M [H,0") - [H,0"] - b) d) pH pH pOH = 9.8 рона (OH)...
5. Which of the following species is amphiprotic in aqueous solution? (a) CH3NH2 c) NH4 (e) HSO (d) F (b) Н:0" 6, Use Table 15.2 (page 529) to decide whether the species on the left or those on the right are favored by the reaction. a. NH4 (aq) + H2PO4" (aq) # NH3(aq) + HsPO b. HCN (aq) + HS(aq) CN" (aq) +H2S c. HCO +OH CO2 H2S d. Al(H20)6 3+ +OH = Al(H20) s2+ OH 7. The equilibrium constant...
my Nules || Ask Your Teac The concentration of hydroxide ions in an aqueous solution is 3.8x109 M. What is the concentration of hydronium ions in this solution at 25°C? M Need Help? 2. - 3 points WAS OSGENCHEM1 14.1.WA.017. My Notes Ask Your Teache Calculate the concentration of the hydroxide ion (OH) in an aqueous solution if the hydronium ion (H20) concentration is 4.98 x 10 Kw - [H,0*1(OH) - 1.01x10-14 at 25°C. moll mol/L. The lon-product constant for...
Which statements listed below can explain why a chemical reaction does not take place? concentration of reactants is too low the temperature is too low not enough effective collisions are occurring some of these answers all of these answers For a chemical reaction the rate of the forward reaction is at a maximum when when the concentration of the reactants and products is the same a state of equilibrium is reached the reaction begins the concentration of products is greater...
3. i). Write the formula of four strong acids and four strong bases. ii). List four factors that affect the strength of an acid. iii). Predict the relative strength of the following compounds: H2O, H2S and H2Se. iv). Which of the following is the stronger acids: CHCICOOH or CHCI-COOH? Explain. v). Al 3* is not a Bronsted acid, Al(H2O)" is. Explain. vi). All Bronsted acids are Lewis acids, but the reverse is not true. Give two examples of two Lewis...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
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