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A 24.5 mL sample of...
A buffer solution is made that is 0.463 M in H2S and 0.463 M in NaHS....
A buffer solution is made that is 0.463 M in H2S and 0.463 M in NaHS. If Kal for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.129 mol HI is added to 1.00 L of the buffer solution instead of H (Use the lowest possible coefficients. Omit states of matter. Use H30 Submit Answer Retry Entire Group 9 more group attempts remaining...
please i need help with these questions... thanks so much Use the References to access important...
please i need help with these questions... thanks so
much
Use the References to access important values if needed for this question. How many grams of solid ammonium chloride should be added to 1.00 L of a 0.174 M ammonia solution to prepare a buffer with a pH of 9.850 ? Breg grams ammonium chloride = 2reg 2reg Submit Answer Retry Entire Group 4 more group attempts remaining A 49.5 ml sample of a 0.302 M aqueous acetic acid solution...
1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate. If 0.180...
1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate. If 0.180 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) A. The number of moles of CH3COOH will remain the same. B. The number of moles of CH3COO- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase....
Please explain how to get the net ionic equations. A buffer solution is made that is...
Please explain how to get the net ionic equations.
A buffer solution is made that is 0.464 M in HCN and 0.464 M in KCN. If Ka for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.115 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made...
this is part a,b,c of one question. please answer all parts or leave to another tutor....
this is part a,b,c of one question. please answer all parts or
leave to another tutor.
Which of the following aqueous solutions are good buffer systems? 0.14 M acetic acid + 0.20 M potassium acetate 0.16 M calcium hydroxide + 0.22 M calcium bromide 0.29 M hydrobromic acid + 0.16 M potassium bromide 0.33 M ammonia + 0.32 M ammonium nitrate 0.38 M barium chloride + 0.26 M barium perchlorate A buffer solution is made that is 0.320 M in...
Part A) A buffer solution is made that is 0.304 M in H2CO3 and 0.304 M...
Part A) A buffer solution is made that is 0.304 M in H2CO3 and 0.304 M in NaHCO3. If Ka1 for H2CO3 is 4.20 x 10^-7 , what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) PART B) A buffer solution is made that is 0.311 M...
34/35 A buffer solution is made that is 0.411 M in HClO and 0.411 M in Nacio. If K, for HCIO is 3.50 x 10-8, w...
34/35
A buffer solution is made that is 0.411 M in HClO and 0.411 M in Nacio. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.122 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made that is 0.365 M in HCN and 0.365...
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS....
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS. Kal If for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.112 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+) + +
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS....
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS. Kal If for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.112 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+) + +
A buffer solution is made that is 0.468 Min H, CO3 and 0.468 M in NaHCO3...
A buffer solution is made that is 0.468 Min H, CO3 and 0.468 M in NaHCO3 . If Kal for H,CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH=) Write the net ionic equation for the reaction that occurs when 0.133 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
A buffer solution is made that is 0.463 M in H2S and 0.463 M in NaHS. If Kal for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.129 mol HI is added to 1.00 L of the buffer solution instead of H (Use the lowest possible coefficients. Omit states of matter. Use H30 Submit Answer Retry Entire Group 9 more group attempts remaining...
please i need help with these questions... thanks so
much
Use the References to access important values if needed for this question. How many grams of solid ammonium chloride should be added to 1.00 L of a 0.174 M ammonia solution to prepare a buffer with a pH of 9.850 ? Breg grams ammonium chloride = 2reg 2reg Submit Answer Retry Entire Group 4 more group attempts remaining A 49.5 ml sample of a 0.302 M aqueous acetic acid solution...
Please explain how to get the net ionic equations.
A buffer solution is made that is 0.464 M in HCN and 0.464 M in KCN. If Ka for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.115 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made...
this is part a,b,c of one question. please answer all parts or
leave to another tutor.
Which of the following aqueous solutions are good buffer systems? 0.14 M acetic acid + 0.20 M potassium acetate 0.16 M calcium hydroxide + 0.22 M calcium bromide 0.29 M hydrobromic acid + 0.16 M potassium bromide 0.33 M ammonia + 0.32 M ammonium nitrate 0.38 M barium chloride + 0.26 M barium perchlorate A buffer solution is made that is 0.320 M in...
34/35
A buffer solution is made that is 0.411 M in HClO and 0.411 M in Nacio. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.122 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made that is 0.365 M in HCN and 0.365...
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS. Kal If for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.112 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+) + +
A buffer solution is made that is 0.445 M in H2S and 0.445 M in KHS. Kal If for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.112 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30+ instead of H+) + +
A buffer solution is made that is 0.468 Min H, CO3 and 0.468 M in NaHCO3 . If Kal for H,CO3 is 4.20 x 10-7, what is the pH of the buffer solution? pH=) Write the net ionic equation for the reaction that occurs when 0.133 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
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